New Observations on the Copper-to-Silver-to-Gold DemonstrationDorin Bejan, Jeff Hastie, and Nigel J. BunceThis analysis of the classic copper-to-silver-to-gold demonstration describes the deposition of zinc in the form of the silver-colored alloy ?-brass, the evolution of hydrogen at the copper cathode, and the behavior of the associated electrochemical cell.Bejan, Dorin; Hastie, Jeff; Bunce, Nigel J. J. Chem. Educ.2008, 85, 1381.

Undergraduates' Understanding of EntropyArnd H. JungermannSzbilir and Bennett carried out an extensive investigation on undergraduates understanding of entropy. Though I agree in general with their statements that orderdisorder arguments form a misleading entropy concept, I would like to make some comments with regard to a certain part of their online supplement.Jungermann, Arnd H. J. Chem. Educ.2008, 85, 1192.

An Inexpensive Solution CalorimeterEmma Kavanagh, Sam Mindel, Giles Robertson, and D. E. Peter HughesDescribes the construction of a simple solution calorimeter, using a miniature bead thermistor as a temperature-sensing element, that has a response time of a few seconds and made it possible to carry out a thermometric reaction in under a minute.Kavanagh, Emma; Mindel, Sam; Robertson, Giles; Hughes, D. E. Peter. J. Chem. Educ.2008, 85, 1129.

Acids / Bases |

Aqueous Solution Chemistry |

Calorimetry / Thermochemistry |

Laboratory Equipment / Apparatus |

Thermal Analysis |

Thermodynamics

Data Pooling in a Chemical Kinetics Experiment: The Aquation of a Series of Cobalt(III) ComplexesRichard S. Herrick, Kenneth V. Mills, and Lisa P. NestorDescribes an experiment that introduces students to integrated rate laws, the search for a mechanism that is consistent with chemical and kinetic data, and the concept of activation barriers and their measurement in a curriculum whose pedagogical philosophy makes the laboratory the center of learning for undergraduates in their first two years of instruction.Herrick, Richard S.; Mills, Kenneth V.; Nestor, Lisa P. J. Chem. Educ.2008, 85, 1120.

EQVAPSIM: A Vapor–Liquid Equilibria of Binary Systems Computer Simulation by LabVIEWA. Belletti, R. Borromei, and G. InglettoReports the results of a program using LabVIEW software to simulate the construction of a phase diagram representing a liquidvapor equilibrium. The program models work in a real laboratory, including mistakes commonly made in this context.Belletti, A.; Borromei, R.; Ingletto, G. J. Chem. Educ.2008, 85, 879.

Understanding the Clausius–Clapeyron Equation by Employing an Easily Adaptable Pressure CookerMonica Galleano, Alberto Boveris, and Susana PuntaruloDescribes a laboratory exercise to understand the effect of pressure on phase equilibrium as described by the ClausiusClapeyron equation. The equipment required is a pressure cooker adapted with a pressure gauge and a thermometer in the lid, allowing the measurement of the pressure and the temperature of the chamber containing the water heated until vaporization.Galleano, Monica; Boveris, Alberto; Puntarulo, Susana. J. Chem. Educ.2008, 85, 276.

Determining the Solubility Product of Fe(OH)3: An Equilibrium Study with Environmental SignificanceMichelle Meighan, Joseph MacNeil, and Renee FalconerThis study explores the environmental impact of acidic mine drainage by investigating the relationship between pH and the aqueous solubility of heavy metals. Students precipitate Fe(OH)3 from acidic FeCl3 and NaOH and use the concentrations of ferric and hydroxide ionsdetermined through pH and flame spectroscopyto calculate the Ksp of Fe(OH)3.Meighan, Michelle; MacNeil, Joseph; Falconer, Renee. J. Chem. Educ.2008, 85, 254.

John KrenosMetiu has created a significant set of volumes on undergraduate physical chemistry. The integration of Mathematica and Mathcad workbooks into the four texts provides instructors with an attractive new option in teaching.Krenos, John. J. Chem. Educ.2008, 85, 206.

Using the Science Writing Heuristic To Improve Students' Understanding of General EquilibriumJames A. Rudd, II, Thomas J. Greenbowe, and Brian M. HandThis study examines the performance of students using the Science Writing Heuristic approach, which facilitates scientific inquiry by structuring the laboratory notebook in a format that guides students to answer directed questions, on lecture exams and a laboratory practical exam on chemical equilibrium.Rudd, James A., II; Greenbowe, Thomas J.; Hand, Brian M. J. Chem. Educ.2007, 84, 2007.

Equilibrium |

Learning Theories |

TA Training / Orientation |

Student-Centered Learning

Origin of the Formulas of Dihydrogen and Other Simple MoleculesAndrew WilliamsThe logic and experimental data are described with which chemists originally deduced the formulas of fundamental substances such as H2, H2O, Cl2, NH3, CH4, and HCl. It is argued that high school and first-year undergraduate students would gain substantially from exposure to this process.Williams, Andrew. J. Chem. Educ.2007, 84, 1779.

Enrichment / Review Materials |

Molecular Properties / Structure

A Simple Calorimetric Experiment That Highlights Aspects of Global Heat Retention and Global WarmingJoel D. Burley and Harold S. JohnstonIn this laboratory experiment, general chemistry students verify that heat is consumed in the melting of ice, with no increase in temperature until all the ice has melted. The fundamental calorimetric principles demonstrated by the lab results are then developed to help students better assess and understand the experimental evidence associated with global warming.Burley, Joel D.; Johnston, Harold S. J. Chem. Educ.2007, 84, 1686.

Redox Titration of Ferricyanide to Ferrocyanide with Ascorbic Acid: Illustrating the Nernst Equation and Beer–Lambert LawTina H. Huang, Gail Salter, Sarah L. Kahn, and Yvonne M. GindtIn this simple experiment, which illustrates the Nernst equation and BeerLambert law, students monitor the reduction of ferricyanide ion to ferrocyanide electrochemically and spectrophoto-metrically upon titration with ascorbic acid. The Nernst equation is used to calculate the standard reduction potential of the redox couple at pH 7 and the number of electrons transferred.Huang, Tina H.; Salter, Gail; Kahn, Sarah L.; Gindt, Yvonne M. J. Chem. Educ.2007, 84, 1461.

Coordination Compounds |

Electrochemistry |

Potentiometry |

Spectroscopy |

UV-Vis Spectroscopy

Exception to the Le Châtelier PrincipleDavid S. Corti and Mark J. UlineDisagreement regarding an apparent exception to the Le Chtelier principle involving the effects of nonideality on the direction in which the ammonia synthesis reaction shifts upon addition of infinitesimal and finite quantities of nitrogen at constant pressure and temperature. Corti, David S.; Uline, Mark J. J. Chem. Educ.2007, 84, 1427.

Equilibrium

Exception to the Le Châtelier PrincipleThomas R. HerrintonDisagreement regarding an apparent exception to the Le Chatelier principle involving the effects of nonideality on the direction in which the ammonia synthesis reaction shifts upon addition of infinitesimal and finite quantities of nitrogen at constant pressure and temperature. Herrinton, Thomas R. J. Chem. Educ.2007, 84, 1427.

Equilibrium |

Gases

Imidazole as a pH Probe: An NMR Experiment for the General Chemistry LaboratoryWilliam J. Hagan, Jr., Dennis L. Edie, and Linda B. CooleyAn experiment is described that employs the 1H-NMR signal of aqueous imidazole to determine the pH of an unknown solution. The procedure involves the preparation of a calibration curve, which is then used for the analysis of the unknown(s).Hagan, William J., Jr.; Edie, Dennis L.; Cooley, Linda B. J. Chem. Educ.2007, 84, 1188.

Mass-Elastic Band Thermodynamics: A Visual Teaching Aid at the Introductory LevelWilliam C. GalleyDemonstrations of five spontaneous isothermal processes involving the coupling of a mass and elastic band and arising from combinations of enthalpy and entropy changes are presented and then dissected. Analogies are drawn between these processes and common spontaneous molecular events such as chemical reactions and phase transitions.Galley, William C. J. Chem. Educ.2007, 84, 1147.

Calorimetry / Thermochemistry |

Thermodynamics

Defining and Teaching pHRichard F. BurtonAt an elementary level, pH and the algebra of equilibria can be simply and correctly taught, without logarithms, in terms of the modern, operationally-defined pH scale that underlies laboratory measurement and relates to activities.Burton, Richard F. J. Chem. Educ.2007, 84, 1129.

Acids / Bases |

pH |

Aqueous Solution Chemistry

The Chemistry of Swimming Pool MaintenanceCarl Salter and David L. LanghusThis paper examines the key ideas behind swimming pool chemistry -- the central importance of pH and its effect on chlorine sanitation and calcium carbonate solubility. The paper also reviews the analytical procedures and common practices used to monitor and control pool chemistry or correct problems.Salter, Carl; Langhus, David L. J. Chem. Educ.2007, 84, 1124.

Acids / Bases |

Applications of Chemistry |

Aqueous Solution Chemistry |

Dyes / Pigments |

pH |

Photochemistry |

Precipitation / Solubility |

Water / Water Chemistry

Enthalpy of Vaporization and Vapor Pressures: An Inexpensive ApparatusRubin Battino, David A. Dolson, Michael R. Hall, and Trevor M. LetcherDescribes an inexpensive apparatus for the determination of the vapor pressure of a liquid as a function of temperature for the purpose of calculating enthalpy changes of vaporization. Also described are a simple air thermostat and an inexpensive temperature controller based on an integrated temperature sensor.Battino, Rubin; Dolson, David A.; Hall, Michael R.; Letcher, Trevor M. J. Chem. Educ.2007, 84, 822.

Using Technology To Enhance the Effectiveness of General Chemistry Laboratory CoursesKathleen M. Carvalho-Knighton and Linda Keen-RochaThis paper makes a case for the pedagogical advantages of performing computer-assisted experiments in the general chemistry laboratory by comparing a control group using traditional bench laboratory procedures with an experimental group using LabWorks software. Carvalho-Knighton, Kathleen M.; Keen-Rocha, Linda. J. Chem. Educ.2007, 84, 727.

An Inexpensive Kinetic Study: The Reaction of FD&C Red #3 (Erythrosin B) with HypochloriteMaher M. Henary and Arlene A. RussellStudents use a desktop visible spectrophotometer to quantitatively follow the rate of disappearance of FD&C Red #3 with hypochlorite. The first-order reaction in both dye and bleach yields simple data that students can easily process and graph using spreadsheet software to obtain the rate constant and the rate law.Henary, Maher M.; Russell, Arlene A. J. Chem. Educ.2007, 84, 480.

Applications of Reaction RateKevin CunninghamThis article presents an assignment in which students are to research and report on a chemical reaction whose increased or decreased rate is of practical importance. The assignment is designed to develop and assess a number of valuable skills and understandings, including the ability to write effectively.Cunningham, Kevin. J. Chem. Educ.2007, 84, 430.

Catalysis |

Enzymes |

Kinetics |

Rate Law |

Reactions |

Applications of Chemistry

Thermochemical Analysis of Neutralization Reactions: An Introductory Discovery ExperimentKenneth V. Mills and Louise W. GuilmetteDescribes a guided-inquiry laboratory pedagogy in which students discover chemical concepts in the lab and the instructor uses their pooled data to guide the lecture portion of the course. This method is illustrated by an experiment that reinforces students' understanding of stoichiometry and allows them to discover neutralization reactions and thermochemistry.Mills, Kenneth V.; Guilmette, Louise W. J. Chem. Educ.2007, 84, 326.

Dulong and Petit's Law: We Should Not Ignore Its ImportanceMary Laing and Michael LaingThis article describes two student exercises: the determination of the specific heat of a metal and hence its atomic weight and a graphical study of specific heat versus atomic weight for different groups of metals and the confirmation of Dulong and Petit's law.Laing, Mary; Laing, Michael. J. Chem. Educ.2006, 83, 1499.

Teaching Physical Chemistry Experiments with a Computer Simulation by LabVIEWA. Belletti, R. Borromei, and G. InglettoThis article reports on a computer simulation developed with the software LabVIEW of the physical chemistry experiment regarding the vapor pressure measurements of a pure liquid as a function of temperature, as well as a system of data collecting that emphasizes the similarities between the virtual and real experiment.Belletti, A.; Borromei, R.; Ingletto, G. J. Chem. Educ.2006, 83, 1353.

Useful Work of a ProcessNorman C. CraigAcknowledgment of a flaw in the article, Lets Drive Driving Force Out of Chemistry.Craig, Norman C. J. Chem. Educ.2006, 83, 703.

Bioenergetics |

Biophysical Chemistry |

Calorimetry / Thermochemistry |

Thermodynamics

Useful Work of a ProcessBruno LunelliClarifies a potentially misleading statement in the article, Lets Drive Driving Force Out of Chemistry.Lunelli, Bruno. J. Chem. Educ.2006, 83, 703.

Bioenergetics |

Biophysical Chemistry |

Calorimetry / Thermochemistry |

Thermodynamics

No "Driving Forces" in General ChemistryEvguenii I. KozliakA simple and easy-to-remember explanation, that precipitation of a solid and/or formation of water are driving forces of those reactions or drive them to completion, still occurs among instructors.Kozliak, Evguenii I. J. Chem. Educ.2006, 83, 702.

An Interactive Environmental Science Course for Education Science MajorsSuzanne K. Lunsford and William SlatteryDescribes an interactive environmental modular science course for education science majors preparing to become teachers at the primary and secondary levels. The purpose of the course is to give students experience in inquiry, gathering data, the evaluation of data to understand scientific theory, and the application of inquiry, hands-on methods in the classroom. Lunsford, Suzanne K.; Slattery, William. J. Chem. Educ.2006, 83, 233.

Electropolymerized Conducting Polymer as Actuator and Sensor Device: An Undergraduate Electrochemical Laboratory ExperimentMaría T. Cortés and Juan C. MorenoA trilayer formed by two conducting polymer films sandwiched around an adhesive polymer layer works as actuator and sensor simultaneously. This device can be bent up to 180 and it can be used as a sensing device of physical chemistry parameters such as cell temperature and electrolyte concentration. In this article, it is shown in a didactic way how to electrochemically synthesize ClO4-doped polypyrrole (PPy) films, how to fabricate a trilayer device, and how to evaluate its actuating and sensing capabilities. The required materials are simple and a complicated setup is not necessary. Cortés, María T.; Moreno, Juan C. J. Chem. Educ.2005, 82, 1372.

Rotational Mobility in a Crystal Studied by Dielectric Relaxation Spectroscopy. An Experiment for the Physical Chemistry LaboratoryMadalena S. C. Dionísio, Hermínio P. Diogo, J. P. S. Farinha, and Joaquim J. Moura-RamosIn this article we present a laboratory experiment for an undergraduate physical chemistry course. The purpose of this experiment is the study of molecular mobility in a crystal using the technique of dielectric relaxation spectroscopy. The experiment illustrates important physical chemistry concepts. The background of the experimental technique deals with the concepts of orientational and induced polarization and frequency-dependent relative permittivity (or dielectric constant). The kinetic concepts of temperature-dependent relaxation time, activation energy, and activation entropy are involved in the concept of molecular mobility. Dionísio, Madalena S. C.; Diogo, Hermínio P.; Farinha, J. P. S.; Moura-Ramos, Joaquim J. J. Chem. Educ.2005, 82, 1355.

Kinetics |

Phases / Phase Transitions / Diagrams |

Solids |

Crystals / Crystallography

Synthesis and Physical Properties of Liquid Crystals: An Interdisciplinary ExperimentGerald R. Van Hecke, Kerry K. Karukstis, Hanhan Li, Hansford C. Hendargo, Andrew J. Cosand, and Marja M. FoxThis experiment features an investigative approach designed for the introductory science or engineering major and integrates concepts in the fields of chemistry, biology, and physics. Derived from faculty research interests, this novel experiment gives students the opportunity to draw conclusions from tests performed to illustrate the connection between molecular structure and macroscopic properties. The chemical synthesis of the compounds studied further enhances the connection between molecular structure and macroscopic physical properties. The results of two separate physical measurements, refractometry and absorption spectroscopy, are combined to calculate a microscopic, but very practical, property of chiral nematic liquidsthe pitch of the helix formed in the liquid crystalline phase.Van Hecke, Gerald R.; Karukstis, Kerry K.; Li, Hanhan; Hendargo, Hansford C.; Cosand, Andrew J.; Fox, Marja M. J. Chem. Educ.2005, 82, 1349.

Chirality / Optical Activity |

Crystals / Crystallography |

Molecular Properties / Structure |

UV-Vis Spectroscopy |

Acids / Bases |

Esters |

Physical Properties |

Physical Properties

A Note on Dalton's Law: Myths, Facts, and ImplementationRonald W. Missen and William R. SmithThe treatment of Dalton's law for gas mixtures commonly includes the improper designation "Dalton's law of partial pressures", rather than the correct "Dalton's law of additivity of (pure component) pressures". It also identifies the pure component pressure as the partial pressure, although these are only numerically equal for a mixture of ideal gases. The situation is clarified by examination of an appropriate statement of the law and definitions, eventually in operational form with reference to mixtures of nonideal gases.Missen, Ronald Wi.; Smith, William R. J. Chem. Educ.2005, 82, 1197.

Thermodynamics |

Gases

Some Insights Regarding a Popular Introductory Gas Law ExperimentEd DePierro and Fred GarafaloThis paper alerts readers to a potential source of error in one approach to the Dumas method as it is often practiced in introductory chemistry laboratories. The room-temperature vapor pressures of volatile compounds that might be considered as unknowns for the experiment lead to determined molar masses that are too low. The greater the vapor pressure of the compound, the lower the determined molar mass will be, when compared to the accepted value. DePierro, Ed; Garafalo, Fred. J. Chem. Educ.2005, 82, 1194.

Kinetics of Alcohol Dehydrogenase-Catalyzed Oxidation of Ethanol Followed by Visible SpectroscopyKestutis Bendinskas, Christopher DiJiacomo, Allison Krill, and Ed VitzA two-week biochemistry experiment was introduced in the second-semester general chemistry laboratory to study the oxidation of ethanol in vitro in the presence of the enzyme alcohol dehydrogenase (ADH). This reaction should pique student interest because the same reaction also occurs in human bodies when alcoholic drinks are consumed. Procedures were developed to follow the biochemical reaction by visible spectroscopy and to avoid specialized equipment. The effect of substrate concentration on the rate of this enzymatic reaction was investigated during the first week. The effects of temperature, pH, the specificity of the enzyme to several substrates, and the enzyme's inhibition by heavy metals were explored during the second week. Bendinskas, Kestutis; DiJiacomo, Christopher; Krill, Allison; Vitz, Ed. J. Chem. Educ.2005, 82, 1068.

Enzymes |

Kinetics |

Oxidation / Reduction |

Reactions |

UV-Vis Spectroscopy |

Alcohols |

Biophysical Chemistry |

Food Science

JavaScript Programs To Calculate Thermodynamic Properties Using Cubic Equations of StatePatrick J. BarrieIn this article, two JavaScript programs are described. The first program gives students the choice of five different cubic equations of state and performs calculations for pure substances. The second program predicts vaporliquid equilibrium for binary mixtures using a choice of three modern equations of state and the van der Waals mixing rules.Barrie, Patrick J. J. Chem. Educ.2005, 82, 958.

Enrichment / Review Materials |

Thermodynamics |

Equilibrium

Misconceptions in Sign Conventions: Flipping the Electric Dipole MomentJames W. Hovick and J. C. PolerReexamination of a central concept from the perspective of a new subdiscipline should not introduce misconceptions about that concept. When misconceptions introduced through chemical language can be avoided, we should change the way we speak.Hovick, James W.; Poler, J. C. J. Chem. Educ.2005, 82, 889.

Molecular Properties / Structure |

Noncovalent Interactions

The q/T Paradox: Which "Contains More Heat", a Cup of Coffee at 95°C or a Liter of Icewater?Ed Vitz and Michael J. SchumanIn this demonstration, heat is removed from 10 cm3 of water at ~95C and 42 cm3 of water at ~0C by adding each to a measured sample of liquid nitrogen. The heat removed from the water boils the N2(l), and the quantity of liquid nitrogen that is evaporated by boiling is determined. The quantity of heat that was absorbed is calculated from the heat of vaporization of liquid nitrogen and found to be about 10,000 J in the case of the hot water and 25,000 J in the case of the icewater.Vitz, Ed; Schuman, Michael J. J. Chem. Educ.2005, 82, 856.

Calorimetry / Thermochemistry |

Heat Capacity |

Phases / Phase Transitions / Diagrams |

Thermodynamics

Greenhouse Gases and Non-gray BehaviorJ. C. JonesGreenhouse gases feature in many courses in applied chemistry as well as in courses on environmental science, atmospheric chemistry, and so on. We hear a great deal about such matters from the media. A more classical topic which first-year chemistry students will learn about in the physical chemistry component of their program is the black body concept and the StefanBoltzmann law. Recently in teaching about greenhouse gases to MSc students I have thought of a link between the topical and classical matters that is pedagogically interesting and might be of value to others teaching in this subject area.Jones, J. C. J. Chem. Educ.2005, 82, 837.

Atmospheric Chemistry |

Gases

Teaching pH Measurements with a Student-Assembled Combination Quinhydrone ElectrodeFritz Scholz, Tim Steinhardt, Heike Kahlert, Jens R. Pörksen, and Jürgen BehnertA combination pH electrode that can be assembled by the student is described. It consists of a glass holder and two sensors in the form of rubber stoppers that contain quinhydrone and graphite. The combination electrode is suitable to teach potentiometric measurements, pH measurements, and the interplay of acidbase and redox equilibria. The electrode meets highest safety standards and overcomes the troubles associated with the use of the conventional quinhydrone electrode.Scholz, Fritz; Steinhardt, Tim; Kahlert, Heike; Pörksen, Jens R.; Behnert, Jürgen. J. Chem. Educ.2005, 82, 782.

Heat and Temperature Conductivity of Baths. Author ReplyErik JolingI appreciate the suggestions made by Bruno Lunelli to improve the usefulness of the microscale heater we described. However, for use in secondary schools sand works fine. In spite of the better properties I would not recommend the use of silicone oil with relatively inexperienced 16-year-old pupils since it can be a bit messy. But that is an argument of classroom management, not of chemistry. Joling, Erik. J. Chem. Educ.2005, 82, 381.

Laboratory Equipment / Apparatus |

Laboratory Management |

Microscale Lab

Heat and Temperature Conductivity of BathsBruno LunelliJoling et al. described a convenient microscale heater in their article, A Low-Cost and Timesaving Microscale Heater. Having had the same problem several years ago, initially I adopted substantially the same solution they proposed. But soon it became apparent that the generic sand bath did not provide a satisfactory thermal contact in terms of both heat transfer and temperature uniformity and control.Lunelli, Bruno. J. Chem. Educ.2005, 82, 380.

Laboratory Equipment / Apparatus |

Laboratory Management |

Microscale Lab

Applying Chemical Potential and Partial Pressure Concepts To Understand the Spontaneous Mixing of Helium and Air in a Helium-Inflated BalloonJee-Yon Lee, Hee-Soo Yoo, Jong Sook Park, Kwang-Jin Hwang, and Jin Seog KimIn developing this laboratory, our initial motivation for the analysis of gases in a balloon was to answer simple and basic questions, such as, Why does a helium-charged balloon left in the air always drop in a few days? Is leakage of helium the only cause of the drop? What is the composition of the gas in the balloon when it falls after deflation? Students were intrigued by these questions, too, as they analyzed the variation over time in the composition in a balloon inflated with helium. Using the concepts of partial pressure and chemical potential, the laboratory experiment described effectively investigates the diffusion process and the behavior of gas molecules for teaching these concepts in general and physical chemistry. Lee, Jee-Yon; Yoo, Hee-Soo; Park, Jong Sook; Hwang, Kwang-Jin; Kim, Jin Seog. J. Chem. Educ.2005, 82, 288.

Transport Properties |

Gases |

Mass Spectrometry |

Quantitative Analysis

On the Buoyancy of a Helium-Filled BalloonJohn E. HarrimanIt is shown by expansion of the exponential in the barometric formula that the forces due to pressure acting on a balloon are of the form (PV/RT)Mg and that results agree with those suggested by Archimedes principle. Einstein's equivalence principal provides an answer to what balloons will do in an accelerated car. Harriman, John E. J. Chem. Educ.2005, 82, 246.

Atmospheric Chemistry |

Gases |

Kinetic-Molecular Theory |

Physical Properties

A General Chemistry and Precalculus First-Year Interest Group (FIG): Effect on Retention, Skills, and AttitudesLaura E. Pence, Harry J. Workman, and Mako E. HarutaGeneral chemistry and precalculus have been linked together through the University of Hartford First-Year Interest Program (FIG) as a means of creating an effective learning community of premedical, biology, and chemistrybiology students. The Integrated Learning Blocks that were created allowed each course to retain the majority of its original content and structure while emphasizing and reinforcing concepts that are common to both classes. Pence, Laura E.; Workman, Harry J.; Haruta, Mako E. J. Chem. Educ.2005, 82, 65.

Mathematics / Symbolic Mathematics

Gravimetric Titrations: In Support of Weight Titration TechniquesRichard W. RametteI write in support of the recommendations of Stephen Hawkes on gravimetric titrations. Weight titration techniques are, in my opinion, by far the best way to bring volumetric analysis into the 20th (let alone 21st) century. Ramette, Richard W. J. Chem. Educ.2004, 81, 1715.

The Effect of Ionic Strength on the Solubility of an ElectrolyteJoan D. WilleyThe theory of activity versus concentration is important in industrial, environmental, and biochemistry. The increase in solubility of an electrolyte in a solution of a second electrolyte with no common ions compared with pure water is not an easy concept to grasp because it seems to be counterintuitive. The simple experiment described here illustrates this principle visually and dramatically. Students attempt to dissolve CaSO42H2O (gypsum) in pure water and in 0.25 M NaCl. Willey, Joan D. J. Chem. Educ.2004, 81, 1644.

Aqueous Solution Chemistry |

Quantitative Analysis |

Water / Water Chemistry |

Solutions / Solvents

Using Organic Light-Emitting Electrochemical Thin-Film Devices To Teach Materials ScienceHannah Sevian, Sean Müller, Hartmut Rudmann, and Michael F. RubnerLight-emitting thin films provide an excellent opportunity to learn about principles of electrochemistry, spectroscopy, microscopic structure of the solid state, basic circuits, and engineering design. There is currently strong interest in academic and industrial engineering research centering on developing organic light-emitting devices for applications in flat panel displays. In this educational module, designed for high school or introductory undergraduate courses, students learn how to make a ruthenium-based thin-film device. In the process, they learn about the solid-state electrochemistry at work in the film, as well as the electroluminescence that results when current passes through the device.Sevian, Hannah; Müller, Sean; Rudmann, Hartmut; Rubner, Michael F. J. Chem. Educ.2004, 81, 1620.

Electrochemistry |

Photochemistry |

Materials Science |

Oxidation / Reduction |

Solid State Chemistry

Teaching Entropy Analysis in the First-Year High School Course and BeyondThomas H. BindelA 16-day teaching unit is presented that develops chemical thermodynamics at the introductory high school level and beyond from exclusively an entropy viewpoint referred to as entropy analysis. Many concepts are presented, such as: entropy, spontaneity, the second law of thermodynamics, qualitative and quantitative entropy analysis, extent of reaction, thermodynamic equilibrium, coupled equilibria, and Gibbs free energy. Entropy is presented in a nontraditional way, using energy dispersal. Bindel, Thomas H. J. Chem. Educ.2004, 81, 1585.

Thermodynamics

Calories - Who's Counting? JCE Editorial StaffStudents determine how many calories are released per gram when marshmallows and cashews burn and then compare the quantity of energy available from carbohydrates vs. fats. JCE Editorial Staff . J. Chem. Educ.2004, 81, 1440A.

Calorimetry / Thermochemistry |

Carbohydrates |

Lipids |

Consumer Chemistry |

Food Science |

Nutrition |

Fatty Acids

A Simple, Inexpensive Water-Jacketed Cuvette for the Spectronic 20Jonathan E. Thompson and Jason TingA simple, inexpensive, water-jacketed cuvette for the Spectronic 20 is described. The cuvette and associated flow system can easily be constructed from materials commonly found in an undergraduate chemistry laboratory. As a demonstration of the cuvette's utility, we used the cuvette for the determination of the activation energy for the reaction between crystal violet and hydroxide ion. However, the cuvette may prove useful in a variety of applications in which a sample must be thermostated within a spectrophotometer. Thompson, Jonathan E.; Ting, Jason. J. Chem. Educ.2004, 81, 1341.

"Prompted" Inquiry-Based Learning in the Introductory Chemistry LaboratoryWilliam J. Green, Curtis Elliott, and R. Hays CumminsA general chemistry laboratory that features a combination of traditionally scripted experiments and an inquiry-based, group project is described. As part of their laboratory experience, students were presented with a list of topics and were encouraged to explore these as written or to alter them to fit their own interests. These "prompts" were effective in allowing students to begin their work in a timely manner and, in most cases, to see a project to completion within a single semester. Green, William J.; Elliott, Curtis; Cummins, R. Hays. J. Chem. Educ.2004, 81, 239.

A Simplified Algorithm for Temperature ConversionsVictor G. MossottiI am surprised that those who teach temperature conversion formulas have not introduced the easier-to-retain relationship based on the fact that 40 F is the same temperature as 40 C. Mossotti, Victor G. J. Chem. Educ.2003, 80, 1380.

Playing-Card EquilibriumRobert M. HansonA simple hands-on simulation suitable for either classroom use or laboratory investigation involves using a standard deck of playing cards to explore the statistical aspects of equilibrium. Concepts that can be easily demonstrated include fluctuation around a most probable distribution, Le Chtelier's principle, the equilibrium constant, prediction of the equilibrium constant based on probability, and the effect of sample size on equilibrium fluctuations. Hanson, Robert M. J. Chem. Educ.2003, 80, 1271.

Equilibrium |

Statistical Mechanics |

Thermodynamics

Simulating Chromatographic Separations in the ClassroomCharles A. Smith and F. Warren VillaescusaUsing this classroom simulation, students develop a set of rules used to investigate the effect of flow rate, column dimension, particle size, and mobile/stationary phase affinity on chromatographic separations. While performing the simulation, the concepts of longitudinal and eddy diffusion are dramatically illustrated. Smith, Charles A.; Villaescusa, F. Warren. J. Chem. Educ.2003, 80, 1023.

A Chemically Relevant Model for Teaching the Second Law of ThermodynamicsBryce E. Williamson and Tetsuo MorikawaPresentation of a chemically relevant model that exemplifies many aspects of the second law: reversibility, path dependence, and extrapolation in terms of electrochemistry and calorimetry.Williamson, Bryce E.; Morikawa, Tetsuo. J. Chem. Educ.2002, 79, 339.

Sink or Swim: The Cartesian DiverK. David PinkertonCartesian divers are a quick and simple way to illustrate relationships among pressure, volume, temperature, and buoyancy. The Activity could be used in connection with the concepts of gases and liquids and discussions of Boyle's, Charles's, and the ideal gas laws.Pinkerton, K. David. J. Chem. Educ.2001, 78, 200A.

LUCID: A New Model for Computer-Assisted LearningTroy Wolfskill and David HansonFeatures of LUCID (Learning and Understanding through Computer-based Interactive Discovery) and student assessments of the system.Wolfskill, Troy; Hanson, David. J. Chem. Educ.2001, 78, 1417.

A Strategy for Incorporating Hands-On GC-MS into the General Chemistry Lecture and Laboratory CoursesPerry C. Reeves and Kim L. PamplinStudents use the GC-MS to obtain spectra of the various halobenzenes. This vividly illustrates the differences in isotopic distributions of the halogens and the complications these differences present in calculating molar masses of compounds. The isotopic distribution of iron is then obtained from the mass spectrum of Fe(CO)5, and the students calculate the atomic mass of iron from this data. Reeves, Perry C.; Pamplin, Kim L. J. Chem. Educ.2001, 78, 368.

Chromatography |

Isotopes |

Mass Spectrometry |

Gas Chromatography |

Aromatic Compounds

Using a Diode Laser Pointer to Count Drops and Automate Titration SystemsPaul Ogren, Steve Nelson, and Ian HenryA diode laser pointer is used to construct a simple system for recording drops falling from a buret. The drop signal is recorded together with one or more measurement signals by a LabVIEW-based programmable interfacing system. A standard buret is converted to a Mariotte buret to provide a constant drop-addition rate.Ogren, Paul; Nelson, Steve; Henry, Ian. J. Chem. Educ.2001, 78, 353.

Laboratory Computing / Interfacing |

Quantitative Analysis |

Instrumental Methods

Understanding Solubility through Excel SpreadsheetsPamela BrownThis article describes assignments related to the solubility of inorganic salts that can be given in an introductory general chemistry course. These assignments address the need for math, graphing, and computer skills in the chemical technology program by developing skill in the use of Microsoft Excel to prepare spreadsheets and graphs and to perform linear and nonlinear curve-fitting. Brown, Pamela. J. Chem. Educ.2001, 78, 268.

Aqueous Solution Chemistry |

Chemometrics |

Precipitation / Solubility

The Synthesis and Analysis of Copper(I) Iodide. A First-Year Laboratory ProjectLara A. Margolis, Richard W. Schaeffer, and Claude H. YoderThis project provides a convenient preparation of a compound whose identity will not be obvious to students. The analytical procedures illustrate the fundamentals of gravimetric analysis and some basic chemical and physical characteristics of the elements. The analytical data allow students to find the identity of the product by determining its empirical formula.Margolis, Lara A.; Schaeffer, Richard W.; Yoder, Claude H. J. Chem. Educ.2001, 78, 235.

Synthesis |

Oxidation / Reduction |

Stoichiometry |

Gravimetric Analysis |

Qualitative Analysis |

Stoichiometry

The State of Division of Solids and Chemical EquilibriaJoão C. M. Paiva and Victor M. S. GilAn experiment and a computer simulation are presented to address a counterintuitive situation often encountered when teaching chemical equilibria. This is prompted by the question "How can the subdivision of a solid reactant affect the reaction rate and not the composition of the equilibrium state?" Paiva, João C. M.; Gil, Victor M. S. J. Chem. Educ.2001, 78, 222.

A Phthalocyanine Synthesis Group Project for General ChemistryDarren K. MacFarland, Christopher M. Hardin, and Michael J. LoweA group experiment synthesizing phthalocyanine dyes in one step from commercially available starting materials is described. The importance of a metal template is explored. The experiment is suitable for a second-semester general chemistry course.MacFarland, Darren K.; Hardin, Christopher M.; Lowe, Michael J. J. Chem. Educ.2000, 77, 1484.

Aromatic Compounds |

Synthesis |

Organometallics |

UV-Vis Spectroscopy |

Aromatic Compounds

Atomic Absorption Spectroscopy of Calcium in Foodstuffs in Non-Science-Major CoursesKeith S. KosteckaNon-science-major students are introduced to the concept of ppm, prepare AAS standard solutions, digest foodstuffs in nitric acid, conduct AAS analysis for Ca, determine mass percentage of calcium in the sample, and check calcium levels in various food items on the Internet with a critical eye.Kostecka, Keith S. J. Chem. Educ.2000, 77, 1321.

Atomic Spectroscopy |

Instrumental Methods |

Nonmajor Courses |

Quantitative Analysis |

Food Science

Thermodynamics of Water Superheated in the Microwave OvenB. H. ErnéWater is conveniently heated above its normal boiling point in a microwave oven in a glass microwave oven teapot. Water stops boiling soon after heating is interrupted, but subsequently added rough particles can still act as nucleation centers for a brief, spectacular burst of steam bubbles. The heat to make those steam bubbles obviously comes from the water itself, so that one can conclude that the boiling water was superheated, which is confirmed with a thermometer.Erné, B. H. J. Chem. Educ.2000, 77, 1309.

Thermodynamics |

Phases / Phase Transitions / Diagrams |

Water / Water Chemistry |

Liquids

A Visual Aid in Enthalpy CalculationsSebastian G. CanagaratnaThis article discusses the use of enthalpy-temperature diagrams for reactants and products as a visual aid in the teaching of reaction-enthalpy calculations. By the use of such diagrams the division of the process into a part involving a chemical reaction without a temperature change and a part involving only a temperature change is made visually concrete.Canagaratna, Sebastian G. J. Chem. Educ.2000, 77, 1178.

Thermodynamics |

Calorimetry / Thermochemistry

A New Approach to Teaching Introductory Science: The Gas ModulePamela Mills, William V. Sweeney, Robert Marino, and Sandra ClarksonA lecture/laboratory module about the behavior of gases that is designed to expose students to the process of scientific discovery, not to teach the gas laws per se. The topic of gases is only the medium used to illustrate other important aspects of physical science: how to process experimental data and reduce it to symbolic mathematical relationships, how to evaluate the reliability of experimental data, and how to view the relationship between experimental data and scientific models. Mills, Pamela A.; Sweeney, William V.; Marino, Robert; Clarkson, Sandra. J. Chem. Educ.2000, 77, 1161.

Paradoxes, Puzzles, and Pitfalls of Incomplete Combustion DemonstrationsEd VitzPaper is burned in a closed container containing sufficient oxygen to consume all the paper. Paradoxically, the flame expires while half of the paper remains. This demonstrates that thermodynamics or stoichiometry is insufficient to explain everyday chemical processes, and that kinetics is often necessary. The gases in the container are analyzed by GC before and after combustion, and the results are examined in detail. Vitz, Ed. J. Chem. Educ.2000, 77, 1011.

Gases |

Kinetics |

Stoichiometry

Studying Thermally Induced Chemical and Physical Transformations in Common Synthetic Polymers: A Laboratory ProjectSteven C. Hodgson, John D. Orbell, Stephen W. Bigger, and John ScheirsA simple project is described for introducing students to some experimental procedures commonly used to measure the effects of thermal treatment on synthetic polymers. The thermally induced changes that occur in the commodity polymers low-density polyethylene (LDPE), poly(ethylene terephthalate) (PET), and poly(vinyl chloride) (PVC) are examined as a function of the time of thermal treatment in an air-circulating oven.Hodgson, Steven C.; Orbell, John D.; Bigger, Stephen W.; Scheirs, John. J. Chem. Educ.2000, 77, 745.

IR Spectroscopy |

Calorimetry / Thermochemistry |

Thermal Analysis |

UV-Vis Spectroscopy

A Closer Look at Phase Diagrams for the General Chemistry CourseStephen A. GramschThe information provided by the high-pressure phase diagrams of some simple systems (carbon dioxide, water, hydrogen, and iron) can provide a useful extension to the traditional discussion of phase diagrams in the general chemistry course. At the same time, it can prepare students for a more illuminating presentation of the concept of equilibrium than is possible through the discussion of gas phase, acid-base, and solubility product equilibria alone. Gramsch, Stephen A. J. Chem. Educ.2000, 77, 718.

Metallurgy in the Laboratory: Preparation of Pure AntimonyBrooke L. O'Klatner and Daniel RabinovichThe preparation of pure antimony is readily accomplished on a laboratory scale by the high-temperature reduction of antimony trioxide with potassium cyanide. The product is obtained in almost quantitative yield (up to 98%) using a procedure that is simple, inexpensive, and quick. O'Klatner, Brooke L.; Rabinovich, Daniel. J. Chem. Educ.2000, 77, 251.

Metals |

Metallurgy

Boerhaave on FireDamon DiementeThis article offers a selection of passages from Boerhaave's chapter on fire. Boerhaave offers demonstrations and experiments that can be instructively performed today, quantitative data that can be checked against modern equations, and much theory and hypothesis that can be assessed in light of modern chemical ideas. Diemente, Damon. J. Chem. Educ.2000, 77, 42.

Calorimetry / Thermochemistry |

Thermodynamics

Microscale Transformations of Some Lead Compounds. A Cycle for Lead Minimizing the Production of WastesFrancisco J. Arnáiz and María R. PedrosaThis set of basic experiments emphasizes that toxic products can be conveniently studied by using a combination of microscale techniques and simple schemes to recycle wastes. Here we propose a basic cycle for lead involving the consecutive transformation of lead(II) acetate to lead(II) formate, lead powder, and lead(II) oxide, with special emphasis on minimizing the production of wastes. Arniz, Francisco J.; Pedrosa, Mara R. J. Chem. Educ.1999, 76, 1687.

Synthesis |

Microscale Lab

Pesticides in Drinking Water: Project-Based Learning within the Introductory Chemistry CurriculumPatricia B. O'Hara, Jon A. Sanborn, and Meredith HowardA new introductory chemistry module is described, which has as its central theme the measurement of trace levels of these xenoestrogens in the form of pesticides in the Town of Amherst's public drinking water. After a basic introduction to sample handling and measurement of pH, temperature, and conductivity, the students travel in small groups to several sites to collect water and perform preliminary characterization of their samples. OHara, Patricia B.; Sanborn, Jon A.; Howard, Meredith. J. Chem. Educ.1999, 76, 1673.

The Solubility of Ionic Solids and Molecular LiquidsC. Baer and Sheila M. AdamusThe solubilities of three ionic salts (NaCl, PbCl2, and KAl(SO4)2.12H2O) in water are measured at four temperatures. The concept of recrystallization is introduced as students cool a high-temperature solution and observe crystal formation. Spreadsheet calculations are performed with the group data, which are then graphed, and students observe the wide variance in solubility behavior for the three salts. Baer, Carl; Adamus, Sheila M. J. Chem. Educ.1999, 76, 1540.

Old Rule of Thumb and the Arrhenius EquationI. A. LeensonThe empirical rule (doubling of the reaction rate upon every 10 increase in temperature) is discussed on the basis of the Arrhenius equation and experimental data. A graph is plotted that shows the applicability limits of the empirical rule in terms of activation energies and temperatures. Leenson, Ilya A. J. Chem. Educ.1999, 76, 1459.

Kinetics

Thermochromism in Commercial ProductsMary Anne White and Monique LeBlancMany commercial products change color with a change of temperature. How do they do it? The processes responsible for the two major categories of commercial thermochromic coloring agents are presented, along with a description of applications of thermochromic materials. White, Mary Anne; LeBlanc, Monique. J. Chem. Educ.1999, 76, 1201.

Acids / Bases |

Consumer Chemistry |

Materials Science |

Applications of Chemistry

An Apparatus for Temperature DisplaysGeorge Papageorgiou and John XenosIn this article, a new simple and low-cost apparatus is introduced that provides the possibility to display temperature measurements in any lecture hall. The apparatus provides analog displays. Its construction requires only simple and inexpensive materials.Papageorgiou, George; Xenos, John. J. Chem. Educ.1999, 76, 1094.

Relative HumidityR. Bruce MartinDaily we hear reports of relative humidity, yet most students remain unfamiliar with its import. This short article defines and describes the concept at several levels. A new, general interest, isobaric plot directly indicates the dependence of relative humidity on temperature. Martin, R. Bruce. J. Chem. Educ.1999, 76, 1081.

Consumer Chemistry |

Gases |

Nonmajor Courses |

Water / Water Chemistry |

Atmospheric Chemistry

Fields of pHPaul Mihas and George PapgeorgiuStudents are taught that the pH of pure water is 7, but the measurement of a sample of distilled water usually gives pH values from 5.5-6.0. In addition, students learn that the ionization of a strong acid determines the pH of an aqueous solution and they cannot distinguish the cases in which ionization of water is significant. Fields of pH was developed to help students overcome such difficulties. Mihas, Paul ; Papgeorgiu, George. J. Chem. Educ.1999, 76, 1032.

Synthesis of Aspirin: A General Chemistry ExperimentJohn A. Olmsted IIIAn experiment is described that is suitable for the early portion of the laboratory in a general chemistry course and integrates organic examples. It is the two-step synthesis of aspirin starting from oil of wintergreen. The mechanism for this synthesis provides examples of three major classes of chemical reactions: hydrolysis, condensation, and proton transfer.Olmsted, John A., III. J. Chem. Educ.1998, 75, 1261.

Drugs / Pharmaceuticals |

Medicinal Chemistry |

Mechanisms of Reactions |

Aromatic Compounds |

Carboxylic Acids |

Aldehydes / Ketones

Why the Arrhenius Equation Is Always in the "Exponentially Increasing" Region in Chemical Kinetic StudiesHarvey F. CarrollThe Arrhenius equation in chemical kinetics, k = Ae-Ea/RT, has, as T gets larger, an inflection point where it changes from an "exponentially increasing" curve to one approaching an asymptote of A. The inflection point occurs at T = Ea/2R. For any activation energy, the inflection point occurs at such a high temperature that chemical kinetic studies would not be possible. Thus, the Arrhenius equation always appears to be exponentially increasing in any chemical kinetic studies of interest. Carroll, Harvey F. J. Chem. Educ.1998, 75, 1186.

Kinetics

The Reaction of a Food Colorant with Sodium Hypochlorite: A Student-Designed Kinetics ExperimentJosefina Arce, Rosa Betancourt, Yamil Rivera, and Joan PijemThe kinetics of the reaction of the food colorant FD&C Blue #1 with sodium hypochlorite (Clorox) is described in a student-designed experimental format. In this format, students are guided- by means of questions- to make decisions regarding concentration of reagents, choice of equipment, and actual laboratory procedures to be followed. Arce, Josefina; Betancourt-Perez, Rosa; Rivera, Yamil; Pijem, Joan. J. Chem. Educ.1998, 75, 1142.

Kinetics |

UV-Vis Spectroscopy |

Dyes / Pigments

An Inexpensive Detector for Gas ChromatographyAllan L. Smith, Edward J. Thorne, and Wolfgang NadlerWe have developed a low-cost (parts cost approximately $70) detector that can be used in a freshman level class to demonstrate the fundamental principles of gas chromatography (GC). The detector box can be used in a modification of experiments available in the literature which do not enable a quantitative method of analysis. We have used it with success in a freshman class of approximately 450 students in an experiment to separate chlorinated hydrocarbons via GC. Smith, Allan L.; Thorne, Edward J.; Nadler, Wolfgang. J. Chem. Educ.1998, 75, 1129.

Chemistry Time: Factors Affecting the Rate of a Chemical ReactionThis activity can be used to introduce a unit on chemical kinetics, but it is simple enough to be used in a discussion of chemical reactions or experimental methods/procedures during the first weeks of the semester. The activity involves reacting bicarbonate with acid, a reaction with practical applications in everyday life.J. Chem. Educ.1998, 75, 1120A.

Kinetics |

Rate Law

Experimentally Determining the Molar Mass of Carbon Dioxide Using a Mylar BalloonBarbara Albers Jackson and David J. CrouseThe molar mass of carbon dioxide was experimentally determined using a Mylar balloon. Mylar balloons are lightweight, have a fixed definite volume, and require minimal additional pressure for inflation. Using the Ideal Gas Equation, the number of moles of air in the balloon was calculated. Jackson, Barbara Albers; Crouse, David J. J. Chem. Educ.1998, 75, 997.

Gases |

Physical Properties

Intermolecular Forces in Introductory Chemistry Studied by Gas Chromatography, Computer Models, and ViscometryJonathan C. Wedvik, Charity McManaman, Janet S. Anderson, and Mary K. CarrollStudents performing gas chromatographic (GC) analyses of mixtures of n-alkanes and samples that simulate crime scene evidence discover that liquid mixtures can be separated rapidly into their components based upon intermolecular forces. Each group of students is given a liquid sample that simulates one collected at an arson scene, and the group is required to determine the identity of the accelerant. Students also examine computer models to better visualize how molecular structure affects intermolecular forces: London forces, dipole-dipole interactions, and hydrogen bonding. Wedvik, Jonathan C.; McManaman, Charity; Anderson, Janet S.; Carroll, Mary K. J. Chem. Educ.1998, 75, 885.

Thermal Physics (and Some Chemistry) of the AtmosphereStephen K. LowerAn exploration of how the temperature of the atmosphere varies with altitude can serve as a useful means of illustrating some important principles relating to the behavior of gases and to the absorption and transformation of radiant energy. Lower, Stephen K. J. Chem. Educ.1998, 75, 837.

Atmospheric Chemistry |

Gases

Logic, History, and the Chemistry Textbook: II. Can We Unmuddle the Chemistry Textbook?William B. JensenHow paying attention to whether a subject is being treated at the molar, molecular, or electrical level of discourse can help to eliminate logically-flawed definitions and concepts, help to revise those which are historically outdated, and help to resolve current debates in the educational literature about the relative merits of competing approaches to a given subject. Jensen, William B. J. Chem. Educ.1998, 75, 817.

Learning Theories

Saving Your Students' Skin. Undergraduate Experiments that Probe UV Protection by Sunscreens and SunglassesJames R. Abney and Bethe A. ScalettarThis article describes absorption spectroscopy experiments that illustrate the mechanism of action of sunscreens and sunglasses and that highlight the differences between different products. The experiments are well suited to incorporation into an undergraduate science laboratory and will expose students to absorption phenomena in a familiar context with substantial environmental and medical relevance. Abney, James R.; Scalettar, Bethe A. J. Chem. Educ.1998, 75, 757.

Photochemistry |

UV-Vis Spectroscopy |

Atmospheric Chemistry |

Applications of Chemistry |

Spectroscopy

Demonstrating Electron Transfer and Nanotechnology: A Natural Dye-Sensitized Nanocrystalline Energy ConverterGreg P. Smestad and Michael GratzelA unique solar cell fabrication procedure has been developed using natural anthocyanin dyes extracted from berries. It can be reproduced with a minimum amount of resources in order to provide an interdisciplinary approach for lower-division undergraduate students learning the basic principles of biological extraction, physical chemistry, and spectroscopy as well as environmental science and electron transfer.Smestad, Greg P.; Grtzel, Michael. J. Chem. Educ.1998, 75, 752.

Beginning Calculations in Physical Chemistry (by Barry R. Johnson and Stephen K. Scott)Lisa Emily ChirlianThis workbook is designed to complement rather than supplement existing textbooks. Its format is one of examples followed by closely coordinated exercises that can be worked directly on the pages of the text itself. The first six chapters present material at a level typically covered in (or before) the first year general chemistry course and the final two chapters move into more sophisticated areas at the level considered in upper-level physical chemistry courses.Chirlian, Lisa Emily. J. Chem. Educ.1998, 75, 549.

Mathematics / Symbolic Mathematics |

Enrichment / Review Materials

The First-Day Quiz as a Teaching TechniqueRaymond S. OchsA first-day quiz for students in an advanced chemistry class, presented to them ostensibly as a test of basic knowledge. The important objective of the exercise is to allow students to realize what they don't know about fundamental chemistry, which makes them more receptive to chemical education.Raymond S. Ochs. J. Chem. Educ.1998, 75, 401.

Learning Theories

Teaching Distillation Knowledge: A Video Film about Distillation Bridging a Gap Between Theory and PracticeMartin J. Goedhart, Hanno van Keulen, Theo M. Mulder, Adri H. Verdonk, and Wobbe De VosThe authors observed that first year students hardly used their knowledge of phase theory in the design and performance of distillations. They therefore developed a video in which they confront students with the boiling properties of liquid mixtures.Goedhart, Martin J.; van Keulen, Hanno; Mulder, Theo M.; Verdonk, Adri H.; De Vos, Wobbe. J. Chem. Educ.1998, 75, 378.

Heat Capacity, Body Temperature, and HypothermiaDoris R. KimbroughA finger in and out of water are compared to demonstrate the difference between heat capacities and their effect on body temperature. Kimbrough, Doris R. J. Chem. Educ.1998, 75, 48.

Calorimetry / Thermochemistry |

Thermodynamics

A Note on Covariance in Propagation of UncertaintyEdwin F. MeyerIt is pointed out that whenever both the slope and the intercept are used in calculating a physical quantity from a linear regression, propagation of error must include the covariance as well as the variances. The point is illustrated with a calculation of the boiling point of water from the parameters of the lnP vs 1/T fit. If the covariance is omitted from the propagation of error, the estimate of uncertainty is unreasonably large. Meyer, Edwin F. J. Chem. Educ.1997, 74, 1339.

Chemometrics

Elements of Curriculum Reform: Putting Solids in the FoundationArthur B. EllisUntil recently, solids were a relatively small part of the chemistry curriculum. Helping to close this particular gap between the research and educational enterprises was the objective of the Ad Hoc Committee for Solid-State Instructional Materials, formed in 1990.Ellis, Arthur B. J. Chem. Educ.1997, 74, 1033.

Materials Science |

Solid State Chemistry |

Nanotechnology |

Magnetic Properties

A Simple Laboratory Demonstration of ElectrochromismBertil ForslundA laboratory exercise in which students are asked to construct an electrochromic cell, consisting of a thin, transparent layer of WO3 on a glass plate with a thin, transparent, and conducting surface coating of doped SnO2.Forslund, Bertil. J. Chem. Educ.1997, 74, 962.

Electrochemistry |

Materials Science |

Solid State Chemistry

A General Chemistry Experiment Incorporating Synthesis and Structural DeterminationHal Van RyswykAn experiment for the general chemistry laboratory is described wherein gas chromatography-mass spectroscopy (GC-MS) and diffuse reflectance infrared Fourier transform spectroscopy (DRIFTS) are used to characterize the products of a series of microscale reactions on vanillin.Van Ryswyk, Hal. J. Chem. Educ.1997, 74, 842.

The Thermodynamics of Drunk DrivingRobert Q. ThompsonBiological, chemical, and instrumental variables are described along with their contributions to the overall uncertainty in the value of BrAC/BAC. Thompson, Robert Q. J. Chem. Educ.1997, 74, 532.

Thermodynamics |

Nonmajor Courses |

Forensic Chemistry |

Drugs / Pharmaceuticals |

Applications of Chemistry

Synthesis and Characterization of a Conduction Polymer: An Electrochemical Experiment for General ChemistryRoger K. Bunting, Karsten Swarat, DaJing Yan, Duane FinelloThe electrochemical synthesis of a free-standing film of polypyrrole, using commonly available equipment and materials, is described at a level suitable to application in a general chemistry laboratory. Also described are methods to quantitatively assess the doping level and to characterize the polymer film in terms of its conductivity as a function of temperature. Bunting, Roger K.; Swarat, Karsten; Yan, DaJing; Finello, Duane. J. Chem. Educ.1997, 74, 421.

Electrochemistry |

Conductivity

Sensitivity to Experimental Parameters via SpreadsheetsB. R. SundheimIn spreadsheet computations wherever the functional dependence of calculated results on experimental quantities is obscure, sensitivities may be obtained by testing the effects of variations in relevant inputs. An example is given where Hess' law is explored calorimetrically.Sundhein, B. R. . J. Chem. Educ.1997, 74, 328.

Four Programs for Windows: Abstract of Volume 4D, Number 2: PSL PhotometerSteven D. GammonThe majority of freshman chemistry laboratory programs include experiments that employ visible spectroscopy to teach Beer's law and derive related concentration information. These experiments are often done with a Baush and Lomb Spectronic 20 or Spectronic 21. We have developed an alternative instrument and software that offers significant advantages over the above spectrometers. Gammon, Steven D. J. Chem. Educ.1996, 73, 1077.

Instrumental Methods |

Laboratory Equipment / Apparatus |

Spectroscopy |

Quantitative Analysis

A New Approach to the General Chemistry LaboratoryJoseph F. Bieron, Paul J. McCarthy, and Thomas W. KermisWith the help of a grant from the National Science Foundation, our department has been able to design a new laboratory course built around several guiding principles. The design called for experiments to be grouped in units or clusters. Each cluster has a unifying theme or common thread, which gives some coherence to the experiments. Bieron, Joseph F.; McCarthy, Paul J.; Kermis, Thomas W. J. Chem. Educ.1996, 73, 1021.

First Day in Organic LabChristine K. F. HermannThis experiment is designed to introduce students to the techniques of reflux, distillation, gas chromatography, and the determination of boiling point and melting point during one lab period. J. Chem. Educ.1996, 73, 852.

An Alternative Methodology for General Chemistry Laboratories: Chemical Equivalent of a MetalCarlos M. Bonatti, José L. Zurita, and Horácio N. SólimoProcedure in which students are asked to identify an unknown metal that can react with mineral acids to evolve hydrogen where the students are required to obtain bibliographic information and decide on some aspects of the experimental work.Bonatti, Carlos M.; Zurita, Jose L.; Sclimo, Horacio N. J. Chem. Educ.1995, 72, 834.

Elements of and in the Chemical Literature: An Undergraduate CourseNovick, Sabrina GodfreySynopsis of a descriptive chemistry course designed to familiarize students with the chemistry of the elements, as well as the wide variety of resources containing information on the properties of the elements and their associated compounds; includes examples of homework and other assessments used in the course. Novick, Sabrina Godfrey J. Chem. Educ.1995, 72, 297.

Raoult's Law Is a DeceptionHawkes, Stephen J.Argument that Raoult's law should be omitted from introductory chemistry courses because of limited applicability and usefulness at that level of study.Hawkes, Stephen J. J. Chem. Educ.1995, 72, 204.

Pictorial Analogies XIII: Kinetics and MechanismFortman, John J.Pictorial analogies for first order kinetics, the effect of concentration and temperature on reaction rate, and the requirement for proper molecular orientation for reaction.Fortman, John J. J. Chem. Educ.1994, 71, 848.

Organic Hourglass Inclusions: A Review of Past and Recent Work and a Student ExperimentKahr, Bart; Chow, Jason K.; Peterson, Matthew L.Discussion of the history and utility of organic hourglass inclusions and a recipe for synthesizing a particular system (K2SO4 containing acid fuchsin), the quantification of the dye content, and the observation of its dichroism.Kahr, Bart; Chow, Jason K.; Peterson, Matthew L. J. Chem. Educ.1994, 71, 584.

Measurement scales: Changing Celsius to Kelvin is not just a unit conversion Nordstrom, Brian H.The key to understanding the difference between Celsius and Kelvin lies in the different types of measurement scales. Students may have an easier time manipulating equations (such as gas laws) if they knew the difference between these scales.Nordstrom, Brian H. J. Chem. Educ.1993, 70, 827.

Unknown identification by simple stoichiometryMcCullough, ThomasA simple experiment in which the student can determine the identity of a soluble carbonate salt using one straightforward reaction and gravimetric analysis.McCullough, Thomas J. Chem. Educ.1993, 70, 592.

Revealing the secret of the Arctic bomb Pearson, Earl F.Arctic bombs and hurricanes can appear to be contradictory to gas law concepts commonly taught to chemistry students. While these phenomena can be explained as applications of simple gas laws, the explanations can be more effective if an apparent contradiction is drawn between students' understanding and the observed pressure-temperature relationship in these two examples.Pearson, Earl F. J. Chem. Educ.1993, 70, 315.

A Device to Collect Sediment Cores: And an Experiment for their Chemical AnalysisDel Delumyea, R.; McCleary, Donna L.The chemical and physical characterization of sediments in aquatic systems can be performed at the introductory chemistry level and the experience is appealing and informative for students. This paper describes a device used to gather samples.Del Delumyea, R.; McCleary, Donna L. J. Chem. Educ.1993, 70, 172.

The Density-Specific Gravity ConnectionMcCullough, ThomasThe author responds to a question asked by a student, "why do we use both density and specific gravity..." if the both have the same value.McCullough, Thomas J. Chem. Educ.1993, 70, 46.

Determining the thermal expansion coefficient of gasesLehmann, Jochen K.The authors improved the design of the apparatus and extended the experimental task on a recently published experiment for determining the zero point of the absolute temperature scale.Lehmann, Jochen K. J. Chem. Educ.1992, 69, 943.

Vapor pressure demonstrations using a butane lighterDelumyea, R. DelThe concept of the change of state of matter and particularly the volatitlity of liquids is an important concept taught in introductory chemistry courses.Delumyea, R. Del J. Chem. Educ.1992, 69, 321.

Gases |

Physical Properties |

Liquids |

Phases / Phase Transitions / Diagrams

General chemistry course content.Spencer, J. N.The world has changed but general chemistry has not, except to add more topics.Spencer, J. N. J. Chem. Educ.1992, 69, 182.

Administrative Issues

Enzyme activity: The ping-pong ball torture analogyHelser, Terry L.The author uses this analogy to help students visualize and understand the effect of reaction conditions on the initial rate of an enzyme-catalyzed reaction.Helser, Terry L. J. Chem. Educ.1992, 69, 137.

Enzymes |

Reactions

Principle of extraction of solute by solventGuha, Prabir Kr.; Guha, RatnaAmong the applications of Nernst's distribution law, the most important and interesting one is the extraction of a substance dissolved in one solvent by another solvent, the two solvents being partially miscible or immiscible.Guha, Prabir Kr.; Guha, Ratna J. Chem. Educ.1992, 69, 73.

Does a one-molecule gas obey Boyle's law?Rhodes, GailBecause the kinetic molecular theory provides a plausible explanation for the lawful behavior of gases, it should be treated in enough depth to show students that the theory accounts for all of the important aspects of ideal gas behavior.Rhodes, Gail J. Chem. Educ.1992, 69, 16.

Are we teaching the right things in general chemistry?Kreyenbuhl, Julie A.; Atwood, Charles H.This paper focuses on a study executed to determine which topics are deemed important for the general chemistry curriculum by researchers at the forefront of their fields.Kreyenbuhl, Julie A.; Atwood, Charles H. J. Chem. Educ.1991, 68, 914.

Meeting one challenge for the '90's Fernandez, Jack E.; Worrell, Jay H.It is not necessary to separate courses for majors and nonmajors. There is a current dichotomy in science between the science found in textbooks and the one practiced by researchers.Fernandez, Jack E.; Worrell, Jay H. J. Chem. Educ.1991, 68, 551.

A brief freshman experience in qualitative organic analysisGriswold, John R.; Rauner, Richard A.This is an experiment aimed at second semester non-major students. Because such courses attempt to cover so much material in so little time, laboratory experiences must be carefully thought out.Griswold, John R.; Rauner, Richard A. J. Chem. Educ.1991, 68, 418.

Effective homework assistanceDever, David F.An alternative technique that proves to be more effective than the usual strategies employed for assisting students with homework.Dever, David F. J. Chem. Educ.1991, 68, 189.

Chemical equilibrium: I. The thermodynamic equilibrium constantGordus, Adon A.This is the first article in a series of eight that investigates the various assumptions that result in the simplified equilibrium equations found in most introductory texts. In this first article, the author considers the general nature of the constant K, Le Chatelier's principle, and the effect of the temperature on K.Gordus, Adon A. J. Chem. Educ.1991, 68, 138.

Thermodynamics |

Equilibrium

Using the Apple game port to measure pHKelly, EdwardA circuit that measures electrical potential using the pushbutton and annunciator connections at the Apple game port.Kelly, Edward J. Chem. Educ.1990, 67, A254.

Synthesis of a phenol-formaldehyde thermosetting polymerBedard, Y.; Riedl, B.Procedure that allows for the synthesis of a 50% aqueous solution of a prepolymer that, with the proper application of heat and pressure, can be used to bind together wood or other materials.Bedard, Y.; Riedl, B. J. Chem. Educ.1990, 67, 977.

A simple second-order kinetics experimentWeiss, Hilton M.; Touchette, KimThe reaction studied in this experiment is the (reversible) dimerization of 2,5-dimethyl-3,4-diphenylcyclopentadienone; the monomer is colored while the dimer is not, so monitoring the reaction with a simple spectrophotometer provides the concentration of the monomer and therefore the rate of its disappearance.Weiss, Hilton M.; Touchette, Kim J. Chem. Educ.1990, 67, 707.

Kinetics |

Spectroscopy |

Aromatic Compounds

Gravimetric analysis: The synthesis of tin iodideHickling, George G.Preparation of tin(IV) iodide to further students' understanding of quantitative analysis and introduce some new laboratory techniques.Hickling, George G. J. Chem. Educ.1990, 67, 702.

Wet labs, computers, and spreadsheetsDurham, BillThe following is a description of some commonly encountered experiments that have been modified for computerized data acquisition.Durham, Bill J. Chem. Educ.1990, 67, 416.

Laboratory Computing / Interfacing |

Nuclear / Radiochemistry |

Titration / Volumetric Analysis |

Calorimetry / Thermochemistry |

Kinetics |

Electrochemistry

A small scale equilibrium experiment Flash, PatrickAn alternative method for the experiment in which the equilibrium constant for the iron-thiocyanate complex is determined.Flash, Patrick J. Chem. Educ.1990, 67, 341.

Happy and unhappy balls: Neoprene and polynorborneneKauffman, George B.; Mason, Stewart W.; Seymour, Raymond B.A new scientific novelty that can be used to demonstrate a number of scientific principles, either in lecture demonstration or laboratory experiments, is a pair of solid, black, identically appearing spheres.Kauffman, George B.; Mason, Stewart W.; Seymour, Raymond B. J. Chem. Educ.1990, 67, 198.

Physical Properties

Copper dissolution in nitric acid Stairs, Robert A.Previous correspondence on the stoichiometry of the dissolution of copper in nitric acid is confused as a result of the attempt to write a single equation.Stairs, Robert A. J. Chem. Educ.1990, 67, 184.

Chemistry: A Search to Understand (Harrison, Anna J.; Weaver, Edwin S.)Walker, B.F.This book is based on materials developed over a period of years for a one-semester course for general students who are envisioned by the authors as "intellectually curious but not professionally driven to develop technical competence in chemistry".Walker, B.F. J. Chem. Educ.1989, 66, A155.

Ferrimagnetism Knox, KerroIt is possible in a simple lecture demonstration to synthesize Fe3O4 right before student's eyes and to show its interaction with a magnetic field, comparing it to a paramagnetic material.Knox, Kerro J. Chem. Educ.1989, 66, 337.

Accurate equations of state in computational chemistry projectsAllbee, David; Jones, Edward101. This article presents one method that allows students to become familiar with the use of modern equations of state and also enhances their understanding of how computers can be used in the study and application of chemistry. [Includes "Editor's note: Changes in the computer series", by Lagowski, J. J., p. 226]Allbee, David; Jones, Edward J. Chem. Educ.1989, 66, 226.

Teaching stoichiometry Figueira, Alvaro RochaStudents have a hard time with stoichiometry because it is often presented in a manner that is divorced from content and application.Figueira, Alvaro Rocha J. Chem. Educ.1988, 65, 1060.

An alternative to using the PV = nRT equation Desmarais, GeorgeThis author shares his application of the factor-label method to solving gas problems which involves using the ideal gas constant as the starting point in the relationship.Desmarais, George J. Chem. Educ.1988, 65, 392.

Gases |

Stoichiometry |

Chemometrics

Determining the solubility of Ca(OH)2 using 45Ca as a tracerEdmiston, Michael D.; Suter, Robert W.These authors have developed a simple lab that can be incorporated into freshman chemistry that allows students to understand the power of radiochemistry as an analytical tool as well as gain perspectives about real versus imagined dangers of radioactivity.Edmiston, Michael D.; Suter, Robert W. J. Chem. Educ.1988, 65, 279.

Spectroscopy in large lecture halls Juergens, FredSpectroscopes are impractical to pass out to large lectures. This author submits his strategy for demonstrating both continuous and discontinuous spectra to 350 students in a large lecture hall using large sheets of grating materials with various light sources.Juergens, Fred J. Chem. Educ.1988, 65, 266.

Introductory laboratory exercisesRollinson, Susan WellsA description of exercises used for the first two weeks of General Chemistry that minimize the individual equipment used so as to avoid problems that commonly occur with the fluctuation of course enrollment that happens in the beginning of the semester.Rollinson, Susan Wells J. Chem. Educ.1988, 65, 159.

Thermodynamics and reactions in the dry wayTykodi, Ralph J.In dealing with reactions in the dry way, we can actually "see" in detail the workings of the thermodynamic machinery responsible for moving the reaction in the spontaneous direction. This note presents ideas at the general chemistry level.Tykodi, Ralph J. J. Chem. Educ.1986, 63, 107.

Polymer chemistry for introductory general chemistry coursesPolymer Core Course Committee in General ChemistryThere exists a breadth in what is taught today as General or Introductory Chemistry. This breadth is typically limited by topics covered in popular texts and by specifications described by the ACS Committee on Professional Training. A new committee makes an effort to recommend polymer-related topics that can be added within these limits.Polymer Core Course Committee in General Chemistry J. Chem. Educ.1983, 60, 973.

Industrial Chemistry

Composition of gas hydrates. New answers to an old problemCady, George H.The author provides a discussion on nonstoichiometric crystalline solids as they deserve attention in elementary chemistry courses because they are interesting and increasingly important. Laboratory activities are included.Cady, George H. J. Chem. Educ.1983, 60, 915.

Stoichiometry |

Solids |

Crystals / Crystallography

Dyeing of anodized aluminumGrotz, Leonard C.Anodization of Al is widely practiced in industry to improve the corrosion resistance of articles made of aluminum.Grotz, Leonard C. J. Chem. Educ.1983, 60, 763.

Industrial Chemistry |

Oxidation / Reduction |

Metals |

Dyes / Pigments |

Applications of Chemistry

Computer simulation of elementary chemical kinetics Nase, Martha L.; Seidman, Kurt44. Bits and pieces, 16. The authors have developed several computer programs that simulate chemical kinetics for elementary first and second order processes. These programs can be used to generate kinetic data that can then be analyzed by the student in a variety of ways.Nase, Martha L.; Seidman, Kurt J. Chem. Educ.1983, 60, 734.

Kinetics |

Rate Law

THERMPRO - A thermodynamics program Joshi, Bhairav D.44. Bits and pieces, 16. THERMPRO is an interactive screen-oriented computer program written in BASICA for an IBM-PC with a graphics capability. It represents a general method of calculating standard thermodynamic properties of chemical reactions from heat capacity data for reactants and products.Joshi, Bhairav D. J. Chem. Educ.1983, 60, 733.

Thermodynamics

NH4HC03: a stimulant for learningRichards, R. RonaldStudents, professors, and the literature have all been confused by the unusual dissociation equilibrium of NH4HCO3.Richards, R. Ronald J. Chem. Educ.1983, 60, 555.

Association of ions and fractional crystallization: a general chemistry experimentScaife, Charles W. J.; Dubs, Richard L.The experiment in this article has been used in laboratories for non science majors and for inorganic chemistry. In both cases students attain a good understanding of what it taking place, how the various procedures affect actual concentrations of ions present, and why particular salts crystallize under certain conditions whereas others do not.Scaife, Charles W. J.; Dubs, Richard L. J. Chem. Educ.1983, 60, 418.

Crystals / Crystallography |

Solutions / Solvents

Molecular association and structure of hydrogen peroxideGigure, Paul A.The typical textbook treatment of molecular association and structure of hydrogen peroxide, and the implications of these concepts for the physical properties of hydrogen peroxide tend to be oversimplified and inaccurate.Gigure, Paul A. J. Chem. Educ.1983, 60, 399.

Molecular Properties / Structure |

Physical Properties |

Phases / Phase Transitions / Diagrams |

Hydrogen Bonding

Le Châtelier's principle: the effect of temperature on the solubility of solids in liquidsBrice, L. K.The purpose of this article is to provide a rigorous but straightforward thermodynamic treatment of the temperature dependence of solubility of solids in liquids that is suitable for presentation at the undergraduate level. The present discussion may suggest how to approach the qualitative aspects of the subject for freshman.Brice, L. K. J. Chem. Educ.1983, 60, 387.

Thermodynamics |

Liquids |

Solids |

Chemometrics |

Equilibrium

Getting a "bang" out of chemical kineticsHague, George R., Jr.The kinetics demonstration described in this note has attracted as many as 15,000people to come and watch.Hague, George R., Jr. J. Chem. Educ.1983, 60, 355.

A novel classification of concentration unitsMacCarthy, PatrickConcentration units can be a source of confusion for students. This article presents a treatment on this topic that may help students understand the differences between these units.MacCarthy, Patrick J. Chem. Educ.1983, 60, 187.

Nomenclature / Units / Symbols |

Solutions / Solvents |

Aqueous Solution Chemistry

An effective demonstration of some properties of real vaporsMetsger, D. ScottThe apparatus described in this article has been found by the authors to be the most effective in vividly illustrating the behavior of a nearly ideal gas to first year chemistry students.Metsger, D. Scott J. Chem. Educ.1983, 60, 67.

Laboratory Equipment / Apparatus |

Gases |

Physical Properties |

Solids

Gas chromatography simulation for a TRS-80 Whisnant, David M.36. Bits and pieces, 13. A gas chromatography simulator on a computer helps aid novice users to become accustomed to the instrument.Whisnant, David M. J. Chem. Educ.1983, 60, 46.

Boyle's law - A different viewSharma, B. D.For a fixed mass of gas at constant temperature the energy of the gas is fixed and independent of its pressure and volume.Sharma, B. D. J. Chem. Educ.1982, 59, 827.

A CAI preparation-for-chemistry courseBeatty, James W.; Scott, Earle S.25. Bits and pieces, 9. Program to teach students how to do basic calculations and solve simple problems in chemistry.Beatty, James W.; Scott, Earle S. J. Chem. Educ.1982, 59, 130.

Enrichment / Review Materials

Separation technology: I. Chromatography Mickey, Charles D.This article covers the development of and the many different types of chromatography available and offers a good overview of the powers of this tool of analytical chemistry.Mickey, Charles D. J. Chem. Educ.1981, 58, 997.

Notation for order of additionNiewahner, J. H.The notation described here will enable a student to include in the chemical equation an implied statement regarding the order of addition.Niewahner, J. H. J. Chem. Educ.1981, 58, 461.

Reactions |

Nomenclature / Units / Symbols

Pressure and the exploding beverage container Perkins, Robert R.The question in this article is an extension of exploding pop bottles to illustrate the balancing of a chemical equation, enthalpy, stoichiometry, and vapor pressure calculations, and the use of the Ideal Gas Equation. The question is aimed at the first-year level student.Perkins, Robert R. J. Chem. Educ.1981, 58, 363.

An approximate determination of Avogadro's constantSzll, Thomas; Dennis, David; Jouas, Jean-Pierre; Wong, MabelAn experiment to determine a value for Avogadro's number by determining the relationship between the number of electrons flowing through an acidified solution of water and the number of moles of electrons which reduce hydrogen ions to produce hydrogen gas.Szll, Thomas; Dennis, David; Jouas, Jean-Pierre; Wong, Mabel J. Chem. Educ.1980, 57, 735.

A chemistry lesson at Three Mile IslandMammano, Nicholas J.Teaching principles of general chemistry through references made to the nuclear incident at Three Mile Island.Mammano, Nicholas J. J. Chem. Educ.1980, 57, 286.

Pepsin and antacid therapy: A dilemmaLaswick, Patty H.; Batson, W. BraytonIllustrates some areas of uncertainty in the current literature regarding the mechanism of digestion and presents an experiment that is more consistent with current biochemical research.Laswick, Patty H.; Batson, W. Brayton J. Chem. Educ.1979, 56, 484.

The temperature dependence of the equilibrium constantBurness, James H.This exam question tests a student's ability to derive the temperature dependence of an equilibrium constant not by qualitatively applying Le Chatelier's principle, but by understanding the relationship between the kinetics of the equation and the value of Keq.Burness, James H. J. Chem. Educ.1979, 56, 395.

Bubble pressure and volume. A demonstration experimentChristian, Sherril D.; Enwall, EricAn interesting phenomenon which illustrates several important principles, is the dependence of the size of a soap bubble on pressure. The subject is introduced to the class by the black box experiment presented in this article.Christian, Sherril D.; Enwall, Eric J. Chem. Educ.1978, 55, 536.

Gases |

Surface Science

Pressure calculations Schultz, Charles W.This question requires students to be able to distinguish two kinds of pressure: Boyles law pressure of gas (that depends on volume) from the equilibrium vapor pressure above a liquid (that does not).Schultz, Charles W. J. Chem. Educ.1978, 55, 515.

Gases |

Chemometrics

Variation of radioactive decay ratesWolsey, Wayne C.133. It is stated frequently in introductory chemistry texts that radioactive decay rates are invariant. Students are led to the impression, implicitly, if not explicitly, that changes in chemical form, temperature, pressure, etc. have no effect upon the half-lives of unstable nuclei. This constancy of decay is perhaps true for some particular modes of decay, but by no means is it true for all.Wolsey, Wayne C. J. Chem. Educ.1978, 55, 302.

Nuclear / Radiochemistry |

Thermodynamics

Temperature dependence of Kw Steffel, M. J.The question presented in this note requires the resolution of a conflict between a common sense notion and an isolated fact.Steffel, M. J. J. Chem. Educ.1978, 55, 243.

Synthesis and reactions of a cobalt complex. A project for freshman laboratoryAlexander, John J.; Dorsey, John G.This lab offers first-year students a rare opportunity for interesting discussions with brighter students, for extending the work involved and for conveying some of the excitement of a developing research problem.Alexander, John J.; Dorsey, John G. J. Chem. Educ.1978, 55, 207.

Coordination Compounds |

Diastereomers |

Spectroscopy

General chemistry thermodynamics experimentBeaulieu, Lynn P., CPTAn experiment is outlined here that provides students with an opportunity to do experimental thermodynamics, and to calculate those thermodynamic values which usually cannot be determined with the simple equipment available in a general chemistry laboratory.Beaulieu, Lynn P., CPT J. Chem. Educ.1978, 55, 53.

Hydrogen bonding and heat of solutionFriedman, NormanAn experiment that clearly illustrates the role of hydrogen bond formation and its effect on the heat of solution.Friedman, Norman J. Chem. Educ.1977, 54, 248.

Ammonia synthesis. A simulated laboratory research projectBayless, Philip L.The authors document simulated experiments which are short enough to be programmed on calculators and require students to interpret the data for further interaction with the program and lead to conclusions of economic, environmental or historical significance.Bayless, Philip L. J. Chem. Educ.1976, 53, 318.

A simple system for demonstrations in spectroscopyAlman, David H.; Billmeyer, Fred W., Jr.The system presented here is an easily accessible horizontal working surface and projects both the color and spectrum of the radiation simultaneously.Alman, David H.; Billmeyer, Fred W., Jr. J. Chem. Educ.1976, 53, 166.

Raku: A redox experiment in glassCichowski, Robert S.In this experiment, students are given the opportunity to handle a glass making process, choosing a colorant and exploring possible reduction-oxidation reactions involving the colorant.Cichowski, Robert S. J. Chem. Educ.1975, 52, 616.

Synthesis, properties, and hydrolysis of antimony trichlorideHentz, F. C., Jr.; Long, G. G.Antimony trichloride is prepared in the same manner as Glauber; a chemical equilibrium that was investigated by LeChatelier is examined; and the antimony in the mercuris vitae of Paracelsus is determined.Hentz, F. C., Jr.; Long, G. G. J. Chem. Educ.1975, 52, 189.

Some simple classroom experiments on the Monte Carlo methodPara, A. Foglio; Lazzarini, E.In this present paper some applications of the Monte Carlo method suggested to freshmen in nuclear physics and chemistry courses are described. These applications are concerned with radioactive decay, statistical fluctuation of the decay, the slowing of fast neutrons, and the calculation of the ratio of partial cross sections of certain nuclear reactions.Para, A. Foglio; Lazzarini, E. J. Chem. Educ.1974, 51, 336.

Nuclear / Radiochemistry

A tribute to Sir Ronald NyholmChatt, J.The author has the unhappy task, but proud privilege to pay tribute to a great chemist and good friend in Professor Sir Ronald Nyholm who was tragically killed in a car accident on a December day in 1971.Chatt, J. J. Chem. Educ.1974, 51, 146.

A practical energy experiment or lecture demonstrationGarin, David L.Presents two demonstrations: one involves heating different volumes of water on the same heater and measuring their temperatures; the other involves heating different volumes of water on the same heater and calculating the heat of vaporization.Garin, David L. J. Chem. Educ.1973, 50, 497.

The helix coil transition of DNASteinert, Roger; Hudson, BruceThe design and use of a photometer to detect the transition of DNA from the double helix to random coil form.Steinert, Roger; Hudson, Bruce J. Chem. Educ.1973, 50, 129.

The chemistry of winemaking. An unique lecture demonstrationChurch, L. B.This paper shows that a very complex series of reactions present in the preparation of wine can be used as the focal point to illustrate many other general classes of chemical reactions and physical processes.Church, L. B. J. Chem. Educ.1972, 49, 174.

An introductory experiment on phosphates in detergentsMohrig, Jerry R.Examines the phosphate controversy, the roles of phosphates in detergents, the chemistry of phosphates and their colorimetric determination, and presents an experiment in which the amount of phosphate is measured using two different analytical methods.Mohrig, Jerry R. J. Chem. Educ.1972, 49, 15.

Aqueous Solution Chemistry |

Water / Water Chemistry |

Consumer Chemistry |

Quantitative Analysis |

Applications of Chemistry

An introduction to principles of the solid state. Extrinsic semiconductorsWeller, Paul F.Includes a previous analogy is extended to cover n- and p-type semiconductors and discussions of the concepts of donors and acceptors, donor and acceptor activation energies and the corresponding charge carrier production at various temperatures, and the effects of the presence of both donors and acceptors.Weller, Paul F. J. Chem. Educ.1971, 48, 831.

Solid State Chemistry |

Solids |

Semiconductors

SI units in physico-chemical calculationsNorris, A. C.This article demonstrates how the adoption of SI units affects some of the more important physico-chemical calculations found at the undergraduate level.Norris, A. C. J. Chem. Educ.1971, 48, 797.

Nomenclature / Units / Symbols |

Chemometrics

Let's get the nonscience majors into the lab!Griffin, Roger W., Jr.The author shares his experiences with a successful laboratory course for nonmajors. Experiments which have been carried out include: geometry of molecules, measurements and errors, separation and purification, spectroscopy, chromatography, colored natural products, and dyes.Griffin, Roger W., Jr. J. Chem. Educ.1971, 48, 685.

Nonmajor Courses |

Dyes / Pigments |

Natural Products |

Chromatography |

Separation Science |

Quantitative Analysis |

VSEPR Theory |

Spectroscopy

Polywater. A lesson and opportunity in scienceChristian, P. A.; Berka, L. H.The authors present an intriguing observation and offer outlines of some possible studies that can be undertaken in any adequately equipped high school or college chemistry laboratory.Christian, P. A.; Berka, L. H. J. Chem. Educ.1971, 48, 667.

Water / Water Chemistry |

Solutions / Solvents

A study of the physical and chemical rates of CaCO3 dissolution in HClBassow, Herbert; Hamilton, Doug; Schneeberg, Ben; Stad, BenThe authors describe the experimental procedure and a discussion of results for a study of the physical and chemical rates of CaCO3 dissolution in HCl.Bassow, Herbert; Hamilton, Doug; Schneeberg, Ben; Stad, Ben J. Chem. Educ.1971, 48, 327.

Trimyristin from nutmegFrank, Forrest; Roberts, Theodore; Snell, Jane; Yates, Christy; Collins, JosephThe author proposes the isolation and saponification of trimytistin from nutmeg as an excellent experiment to introduce general chemistry students to laboratory techniques or for use with the organic chemistry course in which case more techniques an be introduces.Frank, Forrest; Roberts, Theodore; Snell, Jane; Yates, Christy; Collins, Joseph J. Chem. Educ.1971, 48, 255.

Computer evaluation of rates experimentKrieger, Albert G.Notes the availability of a Fortran IV computer program for the numerical evaluation of the "Oxidation of Iodide Ion by Persulfate Ion."Krieger, Albert G. J. Chem. Educ.1970, 47, 839.

Reactions |

Kinetic-Molecular Theory |

Oxidation / Reduction

Hydrolysis of benzenediazonium ionSheats, John E.; Harbison, Kenneth G.Presents a more convenient approach to studying the kinetics of the hydrolysis of benzenediazonium ion.Sheats, John E.; Harbison, Kenneth G. J. Chem. Educ.1970, 47, 779.

Aromatic Compounds |

Nucleophilic Substitution |

Kinetics

So-called zeroth law of thermodynamicsRedlich, OttoThe "zeroth law of thermodynamics" elucidates the difference between the axiomatic and the epistemological method; it is neither a law nor a statement of fact but a guideline for checking our description of nature.Redlich, Otto J. Chem. Educ.1970, 47, 740.

Car Won't Start?Nash, Leonard K.; Plumb, Robert C.Examines the questions, "Does the voltage of a battery drop with temperature" and "Does the ability of a battery to deliver current decrease with temperature?"Nash, Leonard K.; Plumb, Robert C. J. Chem. Educ.1970, 47, 382.

Electrochemistry |

Thin Layer Chromatography |

Applications of Chemistry |

Consumer Chemistry |

Electrolytic / Galvanic Cells / Potentials

An alternative to free energy for undergraduate instructionStrong, Laurence E.; Halliwell, H. FrankIt is the purpose of this paper to question the usefulness of the Gibbs function for the student and to propose an alternative based on the use of entropy functions that help the student to focus more sharply on the features of a system that relate to its capacity to change.Strong, Laurence E.; Halliwell, H. Frank J. Chem. Educ.1970, 47, 347.

Thermodynamics

Our freshmen like the second lawCraig, Norman C.The author affirms the place of thermodynamics in the introductory chemistry course and outlines a presentation that has been used with students at this level.Craig, Norman C. J. Chem. Educ.1970, 47, 342.

Thermodynamics

Sealed tube experimentsCampbell, J. A.Lists and briefly describes a large set of "sealed tube experiments," each of which requires less than five minutes to set-up and clean-up, requires less than five minutes to run, provides dramatic results observable by a large class, and illustrates important chemical concepts.Campbell, J. A. J. Chem. Educ.1970, 47, 273.

Thermodynamics |

Crystals / Crystallography |

Solids |

Liquids |

Gases |

Rate Law |

Equilibrium

Cloud Caps on High MountainsStevenson, Philip E.The formation of cloud caps on high mountains illustrates cooling in an adiabatic expansion and the change in vapor pressure of a liquid with temperature.Stevenson, Philip E. J. Chem. Educ.1970, 47, 272.

Atmospheric Chemistry |

Gases |

Applications of Chemistry |

Phases / Phase Transitions / Diagrams |

Thermodynamics

The Methanol LighterBailar, John C., Jr.The methanol lighter illustrates the roles that thermodynamics, kinetics, and catalysis play in determining if a reaction will take place.Bailar, John C., Jr. J. Chem. Educ.1970, 47, 272.

Thermodynamics |

Kinetics |

Catalysis |

Consumer Chemistry |

Applications of Chemistry

A demonstration experiment on partial molar volumesCoch, Juan A.; Lopez, ValentinThe partial molar volume of trichloroacetic acid can be determined by measuring the increase in volume when TCA is dissolved in water at constant temperature and pressure.Coch, Juan A.; Lopez, Valentin J. Chem. Educ.1970, 47, 270.

An introduction to chromatographyGaucher, G. M.The object of this presentation is to serve as a preliminary practical introduction and guide to chromatography.Gaucher, G. M. J. Chem. Educ.1969, 46, 729.

The law of mass actionBerline, Steven; Bricker, ClarkIt is the purpose of this paper to present a derivation of the Law of Mass Action that should have meaning and could be used at an elementary level.Berline, Steven; Bricker, Clark J. Chem. Educ.1969, 46, 499.

Equilibrium |

Rate Law |

Kinetics

Friday experimentsBissey, Jack E.Provides data on an unknown gas and asks readers to determine if it is ideal, as well as its molecular weight and chemical formula.Bissey, Jack E. J. Chem. Educ.1969, 46, 497.

A research approach in the introductory laboratoryWilson, Lauren R.Presents an alternative to artificial "experiments" in which known results are merely confirmed in which students synthesize a series of chloro-ammine and chloro-ethylene-diaminecobalt(III) compounds.Wilson, Lauren R. J. Chem. Educ.1969, 46, 447.

Indirect calorimetry by computer in the general chemistry courseDeMattia, Dennis; Gruhn, Thomas; Gorman, MelDescribes the use of a Fortran IV program to stimulate student interest in the applications and potential of computer techniques in chemistry.DeMattia, Dennis; Gruhn, Thomas; Gorman, Mel J. Chem. Educ.1969, 46, 398.

A chemistry projects laboratorySteinfeld, J. I.Describes several examples of project experiments that have been conducted as part of a chemistry projects laboratory at MIT.Steinfeld, J. I. J. Chem. Educ.1969, 46, 232.

Laboratory experiments for the introductory chemistry courseWalter, Robert I.Short descriptions of introductory experiments, including separations by recrystallization, distillation, and ion exchange; the oxidation of isopropyl alcohol to acetone; and the synthesis of compounds exhibiting geometric isomerism, Walter, Robert I. J. Chem. Educ.1968, 45, 672.

Separation Science |

Ion Exchange

Computer simulation of experimental dataShwendeman, R. H.This note describes some of the techniques in programming used to generate a sufficient variety of experimental data to provide each student with his own set of numbers for analysis in conjunction with the demonstration laboratory.Shwendeman, R. H. J. Chem. Educ.1968, 45, 665.

From stoichiometry and rate law to mechanismEdwards, John O.; Greene, Edward F.; Ross, JohnExamines the rules used by chemists as guidelines in developing mechanisms from stoichiometric and rate law observations. Edwards, John O.; Greene, Edward F.; Ross, John J. Chem. Educ.1968, 45, 381.

Stoichiometry |

Rate Law |

Kinetics |

Mechanisms of Reactions |

Equilibrium |

Reactive Intermediates

The revolution in elementary kinetics and freshman chemistryWolfgang, RichardNew developments in kinetics so fundamentally affect our most elementary conception of chemical change that they must inevitably be reflected in beginning courses in chemistry; includes an outline for freshmen on elementary chemical dynamics.Wolfgang, Richard J. Chem. Educ.1968, 45, 359.

Kinetics |

Rate Law |

Mechanisms of Reactions

A simple and accurate dilatometer for liquidsWagner, Robert E.; Meyer, Edwin F.The density of a liquid as a function of temperature may be readily measured using this dilatometer.Wagner, Robert E.; Meyer, Edwin F. J. Chem. Educ.1968, 45, 349.

The range of validity of Graham's LawsKirk, A. D.It is the purpose of this article to discuss effusion, diffusion, and some related processes and to outline the range of validity of Graham's law.Kirk, A. D. J. Chem. Educ.1967, 44, 745.

Gases |

Transport Properties

Graham's Laws of diffusion and effusionMason, E. A.; Kronstadt, BarbaraThe purpose of this article is to review Graham's laws of diffusion and effusion, offer simple but essentially correct theoretical explanations for both laws, and to present experiments on the diffusion law.Mason, E. A.; Kronstadt, Barbara J. Chem. Educ.1967, 44, 740.

Laboratory demonstration of fractional distillationColeman, H. M.The method described here permits a quick analysis of the several distillates by direct visualization of one of the two components of a binary mixture containing toluene and acetone.Coleman, H. M. J. Chem. Educ.1967, 44, 476.

The use of talc as a tlc adsorbentWalsh, Brother Joseph M.Describes the use of talc as a thin layer chromatography adsorbent, particularly with respect to the separation of flavonoids, sugars, and proteins.Walsh, Brother Joseph M. J. Chem. Educ.1967, 44, 294.

Thin Layer Chromatography |

Chromatography |

Separation Science |

Proteins / Peptides |

Carbohydrates

An experimental approach to the ideal gas lawBreck, W. G.; Holmes, F. W.It is possible to introduce to students the equation of state, PV = nRT, by an experimental method that demonstrates that PV/T remains constant for a given amount of gas.Breck, W. G.; Holmes, F. W. J. Chem. Educ.1967, 44, 293.

Electronegativities and group IVA chemistryPayne, Dwight A., Jr.; Fink, Frank HallThe teacher of inorganic chemistry should present the representative elements of group IVA and their properties as an intellectual and empirical form of investigation rather than as a mere collection of information.Payne, Dwight A., Jr.; Fink, Frank Hall J. Chem. Educ.1966, 43, 654.

The dissolution of tin in solutions of iodineDavies, J. F.; Trotman-Dickenson, A. F.The progress of this reaction can be followed by the loss of weight of a tin disc.Davies, J. F.; Trotman-Dickenson, A. F. J. Chem. Educ.1966, 43, 483.

The enigmatic polymorphism of ironMyers, Clifford E.Unusual and nontypical, elemental iron can provide the impetus for discussing important chemical principles and properties, including basic thermodynamic concepts and the phenomenon and theory of ferromagnetism.Myers, Clifford E. J. Chem. Educ.1966, 43, 303.

The use and misuse of the laws of thermodynamicsMcGlashan, M. L.Examines the first and second laws, the usefulness of thermodynamics, the calculation of equilibrium constants, and what entropy does not mean.McGlashan, M. L. J. Chem. Educ.1966, 43, 226.

Kinetic energies of gas moleculesAherne, John C.The graph representing the distribution of kinetic energy among the molecules of a gas found in many textbooks is incorrect.Aherne, John C. J. Chem. Educ.1965, 42, 655.

Investigation of interaction in the Pb(NO3)2NaClmethanolwater systemNeidig, H. A.The purpose of this investigation is to collect solubility data for lead(II) nitratesodium chloride methanolwater systems from which a microscopic model can be constructed and used to discuss the various types of interactions occurring.Neidig, H. A. J. Chem. Educ.1965, 42, 475.

Two-track introductory chemistryWalter, Robert I.Describes a two-track introductory chemistry program at Haverford College for students who have had no chemistry in high school and those who have had extensive preparation in chemistry.Walter, Robert I. J. Chem. Educ.1965, 42, 201.

Physical chemistry for freshmen: A rigorous introductionHoffman, Morton Z.; Prock, AlfredDescribes the important components of a course at Boston University that presents selected freshmen students with a rigorous introduction to physical chemistry.Hoffman, Morton Z.; Prock, Alfred J. Chem. Educ.1965, 42, 188.

Decolorization of glassDingledy, DavidA common error in general chemistry textbooks is a statement that manganese dioxide decolorizes commercial glass by virtue of its ability to oxidize blue-green iron(II) to yellow-brown iron(III).Dingledy, David J. Chem. Educ.1965, 42, 160.

Maximum work revisited (Letters)Bauman, RobertComments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.Bauman, Robert J. Chem. Educ.1964, 41, 676.

Thermodynamics |

Gases

Maximum work revisited (Letters)Kokes, Richard J.Comments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.Kokes, Richard J. J. Chem. Educ.1964, 41, 675.

Thermodynamics |

Gases

Maximum work revisited (Letters)Bauman, RobertComments on an earlier "Textbook Error" article that considers at length errors in the calculation of work done in compression or expansion of an ideal gas.Bauman, Robert J. Chem. Educ.1964, 41, 675.

A general chemistry experiment on clathratesSawyer, Albert K.Students prepare one of two hydroquinone clathrates, one that traps methanol and another that traps hydrogen sulfide.Sawyer, Albert K. J. Chem. Educ.1964, 41, 661.

A kinetics experiment for first year chemistryShaefer, William P.The exchange of iodine atoms between organic and inorganic iodides serves as a kinetics experiment for first year chemistry.Shaefer, William P. J. Chem. Educ.1964, 41, 558.

Kinetics |

Isotopes |

Rate Law

The oxidation of iodide ion by persulfate ionMoews, P. C., Jr.; Petrucci, R. H.Presents the oxidation of iodide ion by persulfate ion as an ideal reaction to study as part of an experiment on kinetics.Moews, P. C., Jr.; Petrucci, R. H. J. Chem. Educ.1964, 41, 549.

The Carnot cycle and Maxwell's relationsNash, Leonard K.Maxwells equations can be derived from nothing more than the Carnot cycle and the deployment of the simplest plane geometry.Nash, Leonard K. J. Chem. Educ.1964, 41, 368.

Work of compressing an ideal gasBauman, Robert P.In formulating examples of compression problems there should be an explicit statement that the process is reversible, or at least slow.Bauman, Robert P. J. Chem. Educ.1964, 41, 102.

The formation of acetone from acetatesYoung, Jay A.; Taylor, John K.Suggests some research activities based on an article published previously in the Journal.Young, Jay A.; Taylor, John K. J. Chem. Educ.1962, 39, A962.

Undergraduate Research |

Aldehydes / Ketones |

Reactions

IodomercuratesYoung, Jay A.; Taylor, John K.Suggests some research activities based on an article published previously in the Journal.Young, Jay A.; Taylor, John K. J. Chem. Educ.1962, 39, A960.

Undergraduate Research

The preparation of magnesium nitrideYoung, Jay A.; Taylor, John K.Suggests some research activities based on an article published previously in the Journal.Young, Jay A.; Taylor, John K. J. Chem. Educ.1962, 39, A960.

Synthesis |

Undergraduate Research |

Reactions

The chemistry of silverYoung, Jay A.; Taylor, John K.Suggests some research activities based on an article published previously in the Journal.Young, Jay A.; Taylor, John K. J. Chem. Educ.1962, 39, A960.

A simple gas law apparatusCarter, K. N.The apparatus presented here can be used to verify the ideal gas law, determine the vapor pressure of water at an elevated temperature, or determine the number of moles of dry air under two different sets of conditions for comparison.Carter, K. N. J. Chem. Educ.1962, 39, 302.

Heat of reaction and H2SO4 concentration: A general chemistry experimentWolthuis, Enno; Leegwater, Arie; Ploeg, John VanderThis procedure measures the heat of reaction between water and sulfuric acid of various concentrations; this information is used to determine the concentration of an unknown acid sample.Wolthuis, Enno; Leegwater, Arie; Ploeg, John Vander J. Chem. Educ.1961, 38, 472.

The ionization constant of waterDirkse, Thedford P.Some textbooks claim that the ion product constant of water is constant under all conditions at a given temperature.Dirkse, Thedford P. J. Chem. Educ.1961, 38, 260.

Infrared spectroscopy: A chemist's toolPimentel, George C.This paper serves as an introduction to infrared spectroscopy and seeks to explain why it has assumed such an important role in chemistry.Pimentel, George C. J. Chem. Educ.1960, 37, 651.

Color photography of spectraMarquisee, Joseph A.Using a relatively inexpensive spectrograph, students with no previous experience at color photography can turn out beautiful full color transparencies of spectra that can be viewed in less than two hours.Marquisee, Joseph A. J. Chem. Educ.1960, 37, 580.

Determination of solubility: A laboratory experimentWolthuis, Enno; Pruiksma, Arthur B.; Heerema, Robert P.Students are required to determine the solubility of common salts at various temperatures by finding the temperature at which a solution of known composition is saturated.Wolthuis, Enno; Pruiksma, Arthur B.; Heerema, Robert P. J. Chem. Educ.1960, 37, 137.

Precipitation / Solubility |

Quantitative Analysis |

Aqueous Solution Chemistry |

Solutions / Solvents

Vapor pressure determination: An elementary experimentRadley, Edward T.The approximate vapor pressure of low boiling liquids may be estimated by measuring the increase in length of an air column trapped between two short columns of mercury in a uniform diameter tube.Radley, Edward T. J. Chem. Educ.1960, 37, 35.

Gases

PhotosynthesisBassham, J. A.Provides a detailed review of what is known about photosynthesis and recent developments in methods of investigation.Bassham, J. A. J. Chem. Educ.1959, 36, 548.

Potentiometric measurements of equilibria: In general chemistry laboratoryChesick, J. P.; Patterson, Andrew, Jr.The authors describe an experiment in which the solubility product of silver chloride, the ionization constant of the silver-ammonia complex, and the ionization constant of acetic acid can be determined with one afternoon of work.Chesick, J. P.; Patterson, Andrew, Jr. J. Chem. Educ.1959, 36, 496.

Variation of the solubility product constant with ionic strengthCarmody, Walter R.Describes the development of a demonstration of the constancy (under the right conditions) of the concentration solubility product and the effect of particle size on solubility, and an experiment for quantitatively demonstrating the effect of ionic strength on the concentration solubility product.Carmody, Walter R. J. Chem. Educ.1959, 36, 125.

Precipitation / Solubility |

Aqueous Solution Chemistry

Instability of sulfur-potassium chlorate mixture: A chemical viewTanner, Herbert G.Provides two experiments intended to display the chemistry of and safety guidelines associated with the ignition of sulfur-potassium chlorate mixtures, regularly used as a fuel by model rocket enthusiasts.Tanner, Herbert G. J. Chem. Educ.1959, 36, 58.

Radioisotopes on your rooftopLockhart, Luther, B., Jr.The collection, recovery, and measurement of radioactive materials from atomic testing can be done through the use of relatively simple procedures and is a good exercise in tracer chemistry.Lockhart, Luther, B., Jr. J. Chem. Educ.1957, 34, 602.

Letters to the editorLaughton, Paul M.The author offers an alternative interpretation of the relationship between high school science courses and success in college chemistry.Laughton, Paul M. J. Chem. Educ.1957, 34, 311.

Some simple solid modelsCampbell, J. A.Describes the use of hard spheres to illustrate a variety of concepts with respect solids, including closest packing and the effects of temperature and alloying.Campbell, J. A. J. Chem. Educ.1957, 34, 210.

Textbook errors: X. The classification of crystalsMysels, Karol J.The classification of crystals into several systems (e.g., cubic, tetragonal, orthorombic) is generally based in textbooks on a consideration of crystal axes, particularly their relative lengths and direction; this approach usually gives correct assignments but occasionally leads to an error.Mysels, Karol J. J. Chem. Educ.1957, 34, 40.

Crystals / Crystallography |

Solids

Quantitative principles in general chemistryTaylor, Moddie D.Discusses the principles of the one- and two-constant linear relationships, the inverse linear relationship, a general solution of the one-constant linear relationship, development of the concept of absolute temperature, the molecular weight of soluble solids, and Dulong and Petit's rule.Taylor, Moddie D. J. Chem. Educ.1956, 33, 614.

Mathematics / Symbolic Mathematics

The use of colloidal graphite for laboratory demonstrationsSmith, Edward A.Examines the shape of graphite particles, the electrical properties of colloids, the coagulation of colloids, graphite and magnetic orientation, and the electrical conductivity of graphite.Smith, Edward A. J. Chem. Educ.1956, 33, 600.

Colloids |

Conductivity |

Magnetic Properties

A "clock reaction" for a beginning course in college chemistryBlack, Arthur H.; Dodson, Vance H.The reduction of the cerium(IV) ion in aqueous sulfuric acid to the cerium(III) ion with oxalate ion can be followed visually and without special colorimetric devices.Black, Arthur H.; Dodson, Vance H. J. Chem. Educ.1956, 33, 562.

Reactions

The nature of chromatographyCassidy, Harold G.Provides a definition of chromatography and a description of gas chromatography.Cassidy, Harold G. J. Chem. Educ.1956, 33, 482.

Chromatography |

Separation Science |

Qualitative Analysis |

Gas Chromatography

Some aspects of hydrogen bonding in inorganic chemistryGorman, MelThe purpose of this review is to present some of the research which is illustrative of the methods used and the results obtained with a variety of inorganic compounds in which hydrogen bonding is one of the structural features.Gorman, Mel J. Chem. Educ.1956, 33, 468.

Lecture thermometer and voltmeterDutton, Frederic B.A sensitive temperature-indicating device with a reasonable rapid response time that relies on a thermocouple and can be seen by a large group.Dutton, Frederic B. J. Chem. Educ.1955, 32, 478.

Laboratory Equipment / Apparatus

Simulated research for freshmenSummerbell, Robert K.; Lestina, Gregory; King, L. Carroll; Neumann, H. M.Students are given a solution of some ion not covered in the regular identification scheme and asked to identify the ion, adopt or devise a scheme of analysis for an unknown containing the usual scheme of ions plus the one extra ion, and to analyze a couple of rather simple general unknowns that may or may not contain the extra ion.Summerbell, Robert K.; Lestina, Gregory; King, L. Carroll; Neumann, H. M. J. Chem. Educ.1955, 32, 475.

Undergraduate Research |

Qualitative Analysis |

Aqueous Solution Chemistry

The Grignard reagent reaches the freshmanKing, W. Bernard; Beel, John A.A laboratory procedure that allows students to distinguish between the structure of ethanol and dimethyl ether.King, W. Bernard; Beel, John A. J. Chem. Educ.1955, 32, 146.

A student polarimeterNechamkin, HowardDescribes the construction and use of a crude polarimeter suitable for use by students in early chemistry courses.Nechamkin, Howard J. Chem. Educ.1954, 31, 579.

Laboratory Equipment / Apparatus

Le Châtelier's principle and the equilibrium constantMiller, Arild J.Many students of chemistry have difficulty in understanding how the position of equilibrium in a gaseous reaction can change when the pressure is altered, in accordance with Le Châtelier's principle, without causing a corresponding variation in the equilibrium constant.Miller, Arild J. J. Chem. Educ.1954, 31, 455.

Equilibrium |

Reactions |

Gases

A kinetic analogyLemlich, RobertThis analogy, which clearly demonstrates the principles involved in a first-order reaction, is based on Poiseuille's law for the viscous flow of fluids.Lemlich, Robert J. Chem. Educ.1954, 31, 431.

Linear polymerization and synthetic fibersMoncrieff, Robert W.Examines early research in polymers, the synthesis of polyesters and polyamides, the polymerization of hydrocarbons, and condensation and addition polymerization.Moncrieff, Robert W. J. Chem. Educ.1954, 31, 233.

Letters to the editorWescott, Emery N.Points out an error in the referenced article regarding an example of Pearson's square.Wescott, Emery N. J. Chem. Educ.1954, 31, 101.

Solutions / Solvents |

Chemometrics

Chemistry teaching for general educationHered, WilliamDiscusses various techniques for making the introductory chemistry course more supportive of a general education.Hered, William J. Chem. Educ.1953, 30, 626.

Paper chromatography for studentsBlackwell, R. QuentinDescribes a simple method whereby various mixtures can be separated using paper chromatography under a variety of conditions.Blackwell, R. Quentin J. Chem. Educ.1953, 30, 614.

The kinetic structure of gasesSlabaugh, W. H.Describes a model that illustrates the kinetic properties of gases and ii use to demonstrate the effect of temperature changes on the motion of gas particles.Slabaugh, W. H. J. Chem. Educ.1953, 30, 68.

Gases |

Kinetic-Molecular Theory |

Phases / Phase Transitions / Diagrams

An inexpensive thermostatLinke, William F.A simple and surprisingly efficient thermostat can be constructed in minutes using a three-necked flask and a liquid (or mixture of liquids) that boils at a desired temperature.Linke, William F. J. Chem. Educ.1952, 29, 492.

Laboratory Equipment / Apparatus

LettersHackney, J. C.The author elaborates on the source of a fallacy in the calculation of an overall redox potential by combination of two half-cell potentials.Hackney, J. C. J. Chem. Educ.1952, 29, 472.

Qualitative adequacy of phlogistonScott, John HoweThe author illustrates the phlogiston theory and the reasoning of those who used it historically (particularly Scheele) by applying them to several simple chemical reactions.Scott, John Howe J. Chem. Educ.1952, 29, 360.

Reactions

Lecture demonstrations with siliconesSpalding, David P.Offers a series of demonstrations designed to illustrate some of the basic properties of the silicones that make them unusual substances, including their resistance to high and low temperatures, unusual surface properties, and chemical inertness.Spalding, David P. J. Chem. Educ.1952, 29, 288.

Polymerization

Laboratory synthesis in general freshman chemistryHoltzclaw, Henry F., Jr.The author has found that experiments requiring syntheses of compounds stimulate the interest of students remarkably and provides them with much valuable laboratory experience.Holtzclaw, Henry F., Jr. J. Chem. Educ.1952, 29, 95.

A demonstration on the chemistry of colorBunce, Stanley C.; Hammer, Henry F.Describes a series of demonstrations to illustrate and explain the chemistry of color.Bunce, Stanley C.; Hammer, Henry F. J. Chem. Educ.1951, 28, 546.

The lanthanide contraction as a teaching aidKeller, R N.This paper presents a modified form of the atomic volume curve that illustrates graphically the lanthanide contraction; a number of chemical consequences of this effect are also discussed.Keller, R N. J. Chem. Educ.1951, 28, 312.

Transition Elements |

Periodicity / Periodic Table

Making water gas by cracking methanolViertel, William K.Methanol vapor decomposes very readily at about 1000C into carbon monoxide and hydrogen; presents an apparatus for collecting the hydrogen gas generated through this process.Viertel, William K. J. Chem. Educ.1951, 28, 220.